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- Ascorbic acid (H,C,H,O,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 × 10-5 and Ka2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O] = M [HC,H,0] = M [C,H,0;-] = MYou have a buffer solution containing an acid, HA. The pKa of HA is 7.20 and its conjugate base is A- (assume HA is monoprotic). What is the pH of the solution when [HA] = [A- ]? = 7.20 What is the pH of the solution when you have 10x [HA] to [A- ]? What if you have 10x [A- ] to [HA]?Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH;CH,CO,H, pKa=4.874) using the symbols HA and A, and the given pka value for propanoic acid in the expression. pH = + log - Using the equation to calculate the quotient [A-]/[HA] at three different pH values. pH = 5.321 ГА УНА] - pH = 4.079 [А УНА] 3 pH = 4.874 [А УНА] %3
- Use the modified H-H shown below to calculate the blood plasma pH under the following conditions: [HCO3-] = 0.022 M and pCO₂ = 46 mmHg. Provide your answer to two decimal places. Do not enter units. Dissociation Constant pH = 6.1 Bicarbonate (mmol/L) HCO 0.03 x PCO₂ CO₂ Solubility Constant CO₂ Partial Pressure (mmHg)The K, for acetic acid (CH,COOH) is 1.737 × 10-5. What is the pK, for this acid? pKa = Use the calculated pK, to determine the pH at which [CH,COOH] = [CH,COO¯]. %3D pH =Chem. 1A: Acid-Base titration : to determine molar mass of a diprotic ACID : H2A Put a weighing paper on the pan of balance and tare it. Then add 0.1482 g of an unknown diprotic acid. Transfer the acid to a Erlenmeyer flask add 35.0 mL. water and 4 drops phenophethaleine. The color of solution is colorless. Set up a 50.00 mL. buret: wash the buret with tap water twice, with deionized water twice and and the 0.1029 M NAOH(aq). Fill the buret with 0.1029 M NaOH(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Put the Erlenmeyer flask containing the acid and the phenolphethaleine below the buret with 0.1029 M NAOH(aq). Add NaOH(aq) from buret to the Erlenmeyer flask containing the diprotic acid and phenolphethaleine , until the color of the solution turn to pink by adding one or two drops of NaOH(aq). Then stop adding NaOH(aq) from buret and read the final volume of NaOH(aq). Acid-base titration: buret base of known concentration + stopcock acid of unknown…
- Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH₂CH₂CO₂H, PK₁ = 4.874). pH || pK₂ + log. Answer Bank [A] [HA]Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, - log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L-' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kh for ammonia is 1.8 × 10–5. pKa base] pH = pKa +log acid Express your answer to two significant figures and include the appropriate units. Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. • View Available Hint(s) ? X•10n Value mass of NHẠCI = UnitsCalculate the pH of the buffer solution containing 0.527 M potassium acetate and 0.305 M acetic acid. MМ CH;COOK :98.15 мМ СH,COОH : 60.05 Ka = 1.8x 10-5 CH;COOH CH;COO- + H* Upload your answer and solutions here.
- pKa = pH – log([A¯]/[HA]) pKp = pOH – log([BH+]/[B]) Notice that for pKp a conversion from pH to pOH using the equation pH = 14 – pOH will be necessary. Use this procedure to determine the pH, pKa, and pKp values for the following solutions. Match the words to the appropriate blanks in the sentences below. Make certain each sentence is complete before submitting your answer. • View Available Hint(s) Reset Help 7.50 1. An acidic solution with an initial acid concentration of 0.010 mol/L and an equilibrium 1.99 concentration for A- of 1.79 × 10¬ has a pH of . The pKa of the acid is 1.58 4.75 2. An acidic solution with an initial acid concentration of 0.015 mol/L and an equilibrium concentration for A- of 1.02 × 10-2 has a pH of The pKa of the acid is 11.57 3.43 3. A basic solution with an initial base concentration of 0.021 mol/L and an equilibrium 1.66 concentration for BH+ of 1.38 × 10¬2 has a pH of . The pKb of the base is 12.14 4. A basic solution with an initial base concentration…Consider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answerCalculate the change in pH that occurs when 1.10 mmol of a strong acid is added to 100. mL of the solutions listed below. Ka (CH3COOH) = = 1.75 x 10-5 a. 0.0680 M CH3COOH. Change in pH = b. 0.0680 M CH3COONa. Change in pH =