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PKa pH

pH, pKa, and the Henderson-Hasselbalch Equatio

Whenever you see a p in front of a value, like pH, pKa, and pKb, it means you're dealing with a -log of the value following the p. For example, pKa is the -log of Ka. Because of the way the log function works, a smaller pKa means a larger Ka. pH is the -log of hydrogen ion concentration, and so on pKa (of pKz) is de negatieve log van de Kz en die gebruik je bij bijvoorbeeld de formule van Henderson-Hasselbalch: pH = pKz + log [Z-]/[HZ] de pKz is de pH-waarde op een halve titratie dus als je de titratiecurve tekent en je kijkt dan op de helft van de titratie dan is die pH gelijk aan de pKz-waarde Hoe groter de waarde voor pK a, hoe minder het zuur dissocieert (bij een bepaalde pH), dus hoe zwakker het zuur. De pK a waarde geeft bovendien aan bij welke pH de helft van de zuurmoleculen zijn H +-ion heeft afgestaan: Wanneer de pK a van een zuur bekend is, en de pH gemeten is, kan berekend worden welk deel van de zuurmoleculen zijn H + heeft afgestaan

Pharmacology of Local Anesthetic Agents | Musculoskeletal Key

Een vuistregel hiervoor is dat een pK a < 2,5 een slechte pH-voorspelling geeft; een concentratie groter dan 10 mM van zuren met een pK a > 2,5. De pH-voorspelling zal een lichte afwijking geven, het verschil tussen concentratie en activiteit speelt hier een rol. Een ander probleem ontstaat wanneer een bufferoplossing te sterk wordt verdund When the pH is 3.8, over 90 % exist as acetic acid molecules (CH 3 COOH), but at a pH of 5.8, over 90 % exist as acetate ions (CH 3 COO-). Conversely, to change the pH level near the pKa value of an acid, the dissociation status of the acid must be changed significantly, which requires using an extremely large amount of acid or base Deze vergelijking is: pH = pKa + log /, waar is de concentratie van het zuur en is de concentratie van zijn geconjugeerde base na dissociatie. pH is een variabele die afhankelijk is van de concentratie, dus als u de waarde van deze relatie wilt afleiden, moet u de concentraties van het zuur en de geconjugeerde base kennen. Wat zijn pH en pKa A pH indicator is a weak acid or weak base that changes colour in the transition pH range, which is approximately pK a ± 1. The design of a universal indicator requires a mixture of indicators whose adjacent p K a values differ by about two, so that their transition pH ranges just overlap

Begrijp de relatie tussen pH en pKa - greelane

Visit our website for the notes of this lecture: https://knowbeetutoring.wordpress.com/Get private tutoring from anywhere in the world, via your computer, fr.. Main Difference - pKa vs pH. In physical chemistry, pKa and pH are two terms related to the acidity of a system. These are logarithmic values. The easiest way to express and compare very large or very small amounts is to take their logarithmic value. The logarithm gives a simple value which is very easy to handle In de fysische chemie zijn pKa en pH twee termen gerelateerd aan de zuurgraad van een systeem. Dit zijn logaritmische waarden. De eenvoudigste manier om zeer grote of zeer kleine bedragen uit te drukken en te vergelijken, is door hun logaritmische waarde te nemen. De logaritme geeft een eenvoudige waarde die zeer gemakkelijk te hanteren is

Hoe de PKA in titratie te berekenen Een titratie is een chemisch experiment waarbij u druipt - titreer - de ene substantie in de andere met behulp van een glazen buis (buret) en een beker. Bij een zuur-base titratie titreer je een base in een zuur totdat het zijn equivalentiepunt of een neutrale oplossing met een pH van 7 bereikt http://leah4sci.com/aminoacids presents: Zwitterion and Amino Acid Charge given specific pH and pKa ValuesIs your MCAT just around the corner? Grab a free co..

For example, if the pKa of the acid is 4.75, at a pH of 4.75 that acid will exist as 50% protonated and 50% deprotonated. This also means that as the pH rises, more of the acid will convert to the deproton ated state and at some point the pH will be so high that most of the acid will exist in the deprotonated state. Figure 3 Je berekent de pH in een zure oplossing door middel van de concentratie H3O+. De berekening is als volgt: -log(concentratie H3O+) (log is een functie op je rekenmachine) Om de pH van een basische oplossing te berekenen gebruik je concentratie OH-. Met -log(concentratie OH-) bereken je eerst de pOH. de pH bereken je vervolgens met: 14 - pOH. Succes pH and pOH. Because the constant of water, K w is \(1.0 \times 10^{-14}\) (at 25° C), the \(pK_w\) is 14, the constant of water determines the range of the pH scale. To understand what the pK w is, it is important to understand first what the p means in pOH and pH. The addition of the p reflects the negative of the logarithm, \(-\log\). Therefore, the pH is the negative logarithm of the. pH and pKa relationship for buffers. This is the currently selected item. Buffer capacity. Ways to get a buffer solution. Next lesson. Titrations. Video transcript - [Voiceover] We're gonna talk about the relationship between pH and pK_a and buffers

Ka and pKa calculations | Acid Base Equilibrium | from pH

酸度系數(英語:Acid dissociation constant,又名酸解離常數,代號K a 、pK a 、pK a 值),在化學及生物化學中,是指一個特定的平衡常數,以代表一種酸 解離 氫 離子的能力。. 該平衡狀況是指由一種酸(HA)中,將氫離子(即質子)轉移至水(H 2 O)。 水的濃度[H 2 O]是不會在系數中顯示的 -pKa = -pH + log [A-] / [AH] Als we tenslotte aan beide zijden pH en pKa toevoegen: pH = pKa + log [A-] / [AH] Met deze vergelijking kunt u de pH berekenen als u de dissociatieconstante (pKa) en de concentraties van het zuur en de geconjugeerde base kent. Dit artikel is gemaakt met de hulp van sciencing.com De pKa is de pH waarbij beide vormen in gelijke concentraties voorkomen, deze vind je door te bepalen bij welke pH de extinctie van de zure en basische vorm 50% is van de maximale extinctie, deze pH zou voor beide gelijk moeten zijn. Deze is niet, net zoals beryllium al suggereerde,.

正如Ka,pKa,Kb和pKb一樣,pH和pOH是相關的。 如果你知道pH值,你可以計算pOH。 如果你知道一個平衡常數,你可以計算其他的。 關於pH值 . pH是水溶液(水)中氫離子濃度[H +]的量度。 pH值範圍為0至14.低pH值表示酸度,pH = 7為中性,高pH值表示鹼度 In chemistry carbonic acid is a dibasic acid with the chemical formula H 2 CO 3.The pure compound decomposes at temperatures greater than ca. -80 °C. In biochemistry the name carbonic acid is often applied to aqueous solutions of carbon dioxide, which play an important role in the bicarbonate buffer system, used to maintain acid-base homeostasis

How to Determine pH From pKa Sciencin

1.14: Distinguishing between pH and pKa - Chemistry LibreText

Definities van pH, pKa, Ka, pKb en Kb - www

  1. PKA may refer to: . Parkour Amersfoort; Professionally known as: Pen name; Stage persona; pK a, the symbol for the acid dissociation constant at logarithmic scale; Protein kinase A, a class of cAMP-dependent enzymes; Pi Kappa Alpha, the North-American social fraternity; Public key authentication, establishing key authenticity in public-key cryptography.
  2. Applications like Marvin allow the user to calculate the pKa but also display the pH distribution profile, this can be valuable when thinking about absorption from the different regions of the alimentary canal where the pH ranges from 1-3 in the stomach to 7-8 in the ileum
  3. According to this equation, the pKa and pH values of the same system are equal when half of the acid has been dissociated. Since the buffering capacity of a system is its ability to maintain the pH of a solution, the buffer should be selected in which the pKa and pH are very close to each other
  4. Sinds, pH + pOH = 14; De pH-waarde van een basische oplossing kan ook worden berekend. Er zijn pH-meters en pH-papier in laboratoria, waarmee pH-waarden direct kunnen worden gemeten. pH-papier geeft geschatte pH-waarden, terwijl pH-meters nauwkeurigere waarden geven. pKa. Zuurheid is de toestand van een zuur. Dit hangt samen met de mate van.

Verschil tussen pKa en pH / Wetenschap Het verschil

  1. Ka, pKa, Kb en pKb zijn nuttiger om te voorspellen of een soort protonen bij een specifieke pH-waarde zal doneren of accepteren. Ze beschrijven de mate van ionisatie van een zuur of base en zijn echte indicatoren van zuur of basesterkte omdat het toevoegen van water aan een oplossing de evenwichtsconstante niet zal veranderen
  2. pH, pKa, pI and protein charge. Codon table. Bioinformatics Convert distance matrix to phylip format. 25 Oct 2010. What is acidity. Most people know that pH is a measure of acidity, but what is acidity? The.
  3. e pH given pKa for a monoprotic acid, which is an acid that only donates one proton per molecule when placed in aqueous solution. The general equation for a monoprotic acid in aqueous solution is HA_((aq)) rightleftharpoons H_(aq)^(+) + A_(aq)^(-) If you're dealing with a buffer, then you are dealing with a weak acid
  4. From the plot it is also obvious that buffer capacity has reasonably high values only for pH close to pKa value. The further from the optimal value, the lower buffer capacity of the solution. Solution containing only conjugate base (pH 8-10) has buffer capacity of zero, for the higher pH presence of the strong base starts to play an important role
  5. If pKa - pH > 1 then the solution is 99-100% ionized or 99-100% unionized* Slight discrepancy between this statement and formula used for calculator. Formula used indicates solutions would be 90-100% ionized or unionized. These rules were taken from my Nursing 605 course
  6. So the pKa is equal to the negative log of 2.9 times 10 to the negative 16. Let's get out the calculator and let's do that. Negative log of 2.9 times 10 to the negative 16. This gives us 15.54 when we round that. So the pKa of methanol is equal to 15.54. We could write in a pKa column right here, and for methanol it's 15.54
  7. Omdat, pH pOH = 14; pH-waarde van een basische oplossing kan ook worden berekend. Er zijn pH-meters en pH-papieren in laboratoria, die kunnen worden gebruikt om de pH-waarden direct te meten. pH-papier geeft bij benadering pH-waarden, terwijl pH-meters nauwkeurigere waarden geven. pKa. Zuurgraad is de staat van een zuur

Instructions for pH Calculator Case 1. Initial concentrations of components in a mixture are known. For each compound enter compound name (optional), concentration and Ka/Kb or pKa/pKb values. For example: CH3COOH pKa=4.76 c=0.1 HCl pKa=-10 c=0.1 Case 2. Solution is formed by mixing known volumes of solutions with known concentrations Fraction of Labetolol at pH 7.0 Calculated pKa Macro pKa Micro pKa pKa1=7.5 pka2=9.2 pKa1=7.5 pka2=8.8 pKa3=9.1 pka4=7.8 F+ 0.75 0.72 F F0 F- 0.24 0.005 0 0.27 0.01 0 About 85% of marketed drugs contain functional groups that are ionised to some extent at physiological pH (pH 1.5 8) Ik kom er echter niet helemaal uit hoe je nou precies de pKa uit mn gegevens moet berekenen. Ik dacht dat je gewoon bij het buig/equivalentiepunt van de kromme (mbv 2e afgeleide) moest kijken in de oorspronkelijke titratiekurve welke pH erbij hoort Biochemistry/pKa values. From Wikibooks, open books for an open world < Biochemistry. Buffers are essential to biochemical reactions, as they provide a (more or less) stable pH value for reactions to take place under constantly changing circumstances

The titration curve of a weak acid helps to determine the buffering pH which is exhibited around the pKa of that acid. For example, in the case of acetate buffer, the pKa is 4.76. This is the best buffering pH of acetic acid. Besides, at this pH the acetic acid (CH 3 COOH) and acetate ions (CH 3 CO ph (15.0) pka h2oh(dmso) pka pka2o (dmso) h2o (dmso) guanidinium, n+ n+ n n h nh me me me me o2n no2 no2 nh3 nh hn h me2n nh nh r r h h3n + +nh 3 nh3 nh3 o nh o bn o n+ h n+h 2 h n hn nh n h2nn n n nh rnh2 o nh o n h et ph n h o nh o nh o oo o nh o ph n oh ph me 2nnme n+h 2 me nnh2 o ph nhnh2 nso2ph r nh2 26(thf) d.h. ripin, d.a. evans 19-20 9. At pH= PKa you have 50% of each ionized and noin-ionized species. For good separations it is preferable to run at +/- 2 pH units from PKa pH Definition - Basic (alkaline) vs Acidic - Introduction to pH - acidic and basic (alkaline) Phenols, alcohols and carboxylic acids - pKa values - For oxygen containing organic compounds this is given: pKa (the negative logarithm of the acid dissociation constant), molecular structures, molar weights, density and melting and boiling points AMMONIUM EXCRETION Large amounts of H+ can be excreted without extremely low urine pH because pKa of NH3/NH4 + system is very high (9.2) 39. ACID-BASE BALANCE DISTURBANCES Interactions among the Carbonic Acid-Bicarbonate Buffer System and Compensatory Mechanisms in the Regulation of Plasma pH. 40

At a pH above the pKa the acid is deprotonated. If the pH equals the pKa, the acid is 50% protonated and 50% deprotonated. Attribution: Ivy Jose. In BIS2A, we will be looking at the protonation state and deprotonation state of amino acids. Amino acids contain multiple functional groups that can be acids or bases. Therefore their protonation. In addition, when [b]/[a] is 1/10, we will have pH = pKa - 1. Based on this equation, we concluded that any buffer has the most power to show constant pH. Cite. 3 Recommendations pH and pKa calculations used to be prominently tested on the NAPLEX. Nowadays, they come and go. Bottomline, it is always good practice to know how to do these calculations but they are no where. From pH 2 to 5, ristocetin bears two positive charges. The first one is rigidly attached to the peptidic basket; the second one is located on a side sugar that can rotate (Figure 2). As the pH increases, the negative charges of the four phenol groups increase, reaching four full charges at pH 10 (two pH units above the larger phenolic pKa 8) pKa: The negative decadic logarithm of the ionization constant ( K a ) of an acid; equal to the pH value at which equal concentrations of the acid and conjugate base forms of a substance (often a buffer) are present

pH, pKa, Ka, pKb, and Kb Explained - thoughtco

Pka - Wetenschapsforu

$\begingroup$ Yeah but the pKa equals the pH at the H-E point $\endgroup$ - Asker123 May 1 '15 at 23:29 $\begingroup$ But we are talking about an indicator which itself is a weak acid. I understand what you said is correct, for other situations, but isn't exactly what I am looking for. $\endgroup$ - most venerable sir May 1 '15 at 23:3 Tris-HCl (pKa = 8.06) and maleate (pKa = 6.26) have a working range of pH 5.0-8.6 and may be used successfully to buffer staining solutions (e.g., Toluidine Blue O).Avoid Tris with aldehyde fixatives or osmium tetroxide, however, as the aldehydes reacts with the amino group of Tris, resulting in the loss of buffering capacity A pKa Database » equilibrium constants of some 250 acids and bases (see list) have been compiled into a database expandable by the user. » quick load of pKa sets of seven acid-base systems into the pH_calc, Simulation and Regression modules, for simultaneous use Solute pKa, Solvent pH, and Solubility. According to the Henderson-Hasselbach equation, the relationship between pH, pKa, and relative concentrations of an acid and its salt is as follows: where [A-] is the molar concentration of the salt (dissociated species) and [HA] is the concentration of the undissociated acid Looking for online definition of PKA or what PKA stands for? PKA is listed in the World's largest and most authoritative dictionary database of abbreviations and acronyms The Free Dictionar

Using the pKa values, one can see lactic acid is a stronger acid than acetic acid. 16. 16 Its tells us ionised form & unionised form of drug mean its Absorption of drug in systemic circulation. Ex:-If Pka value of drug is equal to PH then the 50% drug is in ionised form & 50% drug Is in Unionised form. Tells us its excretion rate of drug. 17 For a weak base the ratio will be 10(pH - pKa) : 1 . 75% unionized/ 25% ionized, If pKa - pH > 1 then the solution is 99-100% Aminofil? If a patient is given sodium pentothal orally Formula used To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter MoBio > pH and pKa A molecule, or an atom group in a molecule, may lose or gain a proton when the molecule is placed in an aqueous solution. The exact probability that a molecule will be protonated or deprotonated depends on the pK a of the molecule and the pH of the solution A pKa below -2 describes a strong acid that completely dissociates into its ions when added to a solution. Acids with a high pKa, such as sodium bicarbonate, dissociate less. They are known as weak acids. The pKa is used to calculate the pH of an acid or base, which is another calculation to describe the acidity of a compound

Zuurconstante - Wikipedi

Answer to 1.The pKa of HCHO2 is 3.74. What is the pH of a 0.800 M solution of NaCHO2? Question 1 options: 13.2 8.82 8.72 0.322 2.. Aspirin is an orally administered non-steroidal antiinflammatory agent. Acetylsalicylic acid binds to and acetylates serine residues in cyclooxygenases, resulting in decreased synthesis of prostaglandin, platelet aggregation, and inflammation. This agent exhibits analgesic, antipyretic, and anticoagulant properties The pKa values for organic acids can be found in Appendix II of Bruice 5th Ed. Table of Acids with Ka and pKa Values* CLAS * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. The pKa values for organic acids can be found in Appendix II of Bruice 5th Ed. Title: Acid Author. View the profiles of people named Pka Ph. Join Facebook to connect with Pka Ph and others you may know. Facebook gives people the power to share and.. Makes Debye-Huckel corrections for the effect of ionic strength on pKa; Describes two ways (titration or by accurate weight) for preparation of the recipe; Choose the buffer species you want to use, and enter parameters for volume, pH, and concentration of buffer species. Then, include the option to modify the ionic strength by addition of.

Added Mar 27, 2014 by kalexchu in Chemistry. This widget finds the pH of an acid from its pKa value and concentration. Alternatively, it can be used to find the pOH value of a base by inputting its pKb value in the pKa= input field HH equation, pH = pKa + log(1) or pH = pKa. • If more base is added, the conjugate base form becomes greater till the equivalance point when all of the acid is in the conjugate base form. Buffers • Biological systems use buffers to maintain pH pH calculation formula: pH = -log(1/H +) Where: H +: Hydrogen ion concentration in the solution H + concentration of acid is depended on its pKa, for strong acid like HCl, its pKa=1, thus H + concentration of 1 M HCl is also 1 M; for weak acid such as acetic acid, its pKa=0.0000175, thus H + concentration of 1 M acetic acid is: 1 * 0.0000175 = 0.0000175 GALAS Algorithm. The internal training set is comprised of >17,500 compounds representing >20, 000 ionization centres. A database of ionization centres, interaction constants, and interaction calculation methods are used to simulate a complete distribution plot of produce a full range of protonation states of the molecule at different pH conditions. pH dependency of net molecular charge. Ph 30.7 Nitriles pKa (in DMSO) Sulfides pKa (in DMSO) Sulfoxides & Sulfones pKa (in DMSO) Ph S O R R = H R = Ph 33 27.2 S Me Ph Ph 16.3 Ph S R O O R = H R = Ph 29.0 23.4 O CH3 49 Phosphines pKa (in DMSO) Ph3P CH3 22.4 P O EtO EtO R R = Ph R = CN R = CO2Et 27.6 16.4 18.6 Ph2P PPh2 29.9 Nitro pKa (in DMSO) O2N R R = H R = Ph 17.2 12.

pKa = pH + log (acid/base) % acid ( acid / acid + base ) x 100 % base ( base / acid + base ) x 100. log P is a predictor. of lipophilicity. lipophilicity and hydrophilicity influence. absorption, distribution, elimination, and related properties. log P can be calculated by 各种酸的pka及ph值. 各种酸的pka及ph值 pka1 化学式 4.74 (e)-2-己烯酸 h(ch2)3ch═chcooh 4.72 (e)-3-己烯酸 ch3ch2ch═chch2cooh 2.12 1,3,5-苯三甲酸 c6h3(cooh)3 1.89 hc≡ccooh 2-丙炔酸 ch3ch2ch═chcooh4.7 2-戊烯酸 ch2═chch2cooh 4.68 3-丁烯酸 ch3ch═chch2cooh 4.52 3-戊烯酸 ch2═chch2ch2cooh 4.677 4-戊烯酸 ch3chnh2cooh 9.87 a-丙胺酸 ch2nh2ch2cooh 10.

Experimental and Calculated pKa Values of the ACE

Henderson-Hasselbalch-vergelijking - Wikipedi

PH And PKa Temperature If Temperature Changes Then Ka And Kb Changes How To Prepare 20 MM Potassium Phosphate Buffer PH 6.8? Self-association Of Organic Solutes In Solution: A NEXAFS Image detail for Pka Ph : Title: Pka Ph; Date: November 09, 2019; Size: 8kB; Resolution: 581px x 665px; More Galleries of PH And PKa pH calculation questions » finding pKa of weak acid. 20 mL of 0.1 M solution of weak acid was mixed with 8 mL 0.1 M solution of NaOH. Measured pH was 5.12. Calculate pK a.. In the case of not-so-weak acids you can assume the neutralization reaction is quantitative (all of the strong base reacts with the weak acid) and the pH of the solution is described by Henderson-Hasselbalch equation Enter the pKa value into the calculator and divide by 2. The equation for calculating pH is that pH is equal to half the pKa minus half the log (to base 10) of the concentration, or pH = 1/2(pKa) - 1/2 (logC) where C represents the concentration

pKa and Dissociation Equilibrium : SHIMADZU (Shimadzu

A mitochondrial pH sensing fluorescent probe namely 2-(2-(6-hydroxynaphthalen-2-yl)vinyl)-3-(6-(triphenyl-phosphonio)hexyl)benzothiazol-3-ium bromide (HTBT2) was designed and facilely synthesized via the Knoevenagel condensation reaction.HTBT2 displayed a linear fluorescence enhancement at 612 nm in response to pH changes between 8.70 and 7.20. The pK a value was determined to be 8.04 ± 0.02. Use Henderson-Hasselbalch Equation to determine pH for 0.80M HF/0.50M NaF. Henderson-Hasselbalch Equation pH = pKa + log[A-1]/[HA] = -log(3.5x10-4) + log[0.50]/[0.80] = 3.46 + (-0.40) = 3.26 BACK TO MAIN PAG

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Hoe de pH van pKa te bepalen - Wetenschap - 202

Question: You Are Using Formic Acid (pKa = 3.75) To Make 1.0 L Of 75.0 MM Buffer At PH = 3. It Was Determined That [HCOOH] = 0.0637 M And [HCOO-] = 0.0113 M. In Making The Buffer, You Find That You Can Buy 19 M Formic Acid From A Chemical Company Buffer pKa and pH Range Values For preparation of . Buffers in the pH . Buffers pKa range . Hydrochloric Acid - HCl 0-2 . Nitric Acid - HNO. 3 . Perchloric Acid - HClO. 4. Potassium Chloride - KCl 1.1-1.8 . Oxalic Acid - C. 2. H. 2. O.

6Acides faiblesANTI-INFLAMMATOIRES NON STÉROÏDIENS (AINS) - Synthèse etpH Indicators of Acid-Base Indicators for STPM ChemistryWhat do you mean by isoelectric point is a distinctAcidos Y Bases
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