Calculate the pKa for the weak acids that have the ff. Ka values. a. 2.3 x 10 -6 b. 1.9 x 10 -8 C. 6.4 x 10 -12

Please calculate the pH of a buffer solution made up of formic acid and sodium formate. The solution was made by dissolving 0.808 mol of sodium formate, and 0.808 mol of formic acid in 1.80 Liter of water (please assume a total volume for the solution of 1.80 L). (Ka = 1.80 x 10-4) a. pH= 1.93 Ob. pH = 2.11 Oc. pH = 3.08 d. pH = 3.74 QUESTION 2 The Ka for Formic Acid = 1.80 x 10-4. What is the pH of a 0.778 M Formic Acid solution? HA +B+ A + HB+ Oa. pH = 2.11 b. pH = 1.57 c. pH = 1.93 d. pH = 1.81

Choose the letter of the correct answer: 1. Which of the following salts will produce a basic solution upon hydrolysis?a. NH4NO3b. K2SO4c. NaC6H5COOd. NH4ClO4 2. What buffer pH can be prepared from an arbitrary weak acid whose pKa is 7.20?a. pH 8.30b. pH 6.40c. pH 2.80d. pH 5.80 3. All salts are products of neutralization reactions between an acid and a base. Thus, all salts form a neutral solution when dissolved.a. Trueb. False 4. Which source of error will cause an increase in buffer capacity during determination?a. Higher volume of the buffer was usedb. pH meter was read prematurely, resulting to a larger pH changec. Large amounts of the NaOH was added to the buffer with minimal pH changed. Large amounts of water was accidentally spilled into the buffer 5. Ions that are derived from strong acids and bases, which neither has acid nor base propertiesa. Hydrolyzable ionsb. Acidic/Basic ionsc. Spectator ionsd. Neutralizer ions

Let HA represent a weak acid. A 10.0 mL sample of 0.60 M HA was titrated with 0.30 M NaOH. The following data were collected during the titration. Volume NaOH added (mL) 10.00 12.50 20.00 25.00 pH 7.46 7.99 10.31 12.63 What is the Ka for HA? 1.2 x 10-8 1.0 x 10-7 4.9 × 10-11 None of these 3.5 x 10-8

At a temperature of 298K the value of Ka for ethanoic acid is 1.70 * 10Smoldm3. c. Calculate the pH of a solution of ethanoic acid with a concentration of 0.350moldm-3 at 298K. Pentanoic acid is another example of a weak acid. d. Calculate the value of Ka for a solution of O.0500moldm³ pentanoic acid with a pH of 3.05 at a temperature of 298K. Give your answer to an appropriate number of significant figures.

Sodium is prepared by adding 10 mL of 0.1 M acetic acid to 20 mL of 0.1 M sodium acetate. Calculate the pH of sodium. [pKa (acetic acid) = 4.67]. a. 5.04 b. 5.06                   c. 4.48                   d. None of these              e. 4.74

An 8.0 M solution of formic acid (HCOO) ionizes 0.47%. Determine the dissociation constant, Ka, of formic acid. Select one: to. 1.8 x 10-4 b. 2.0 x 10-4 С. 2.2 х 10-4 d. 4.7 x 10-3 and. 9.4 x 10-3

A solution is a mixture of 0.100M weak acid and 0.020M of its conjugate base. The pH of the resulting solution is 5.20. What is the pKa of the weak acid? a. 7.00 b. 4.50 c. 5.90 d. 4.74 e. 8.24

Refer to the following titration curve and answer the following questions. Enter numerical whole value only. PH 12 9 6 3 2 [OH-] eq 3 The number of inflection points: The value of the most basic pKa value:

23. Consider a generic polyprotic acid H2YO3. What is an appropriate combination of acid dissociation constants for this acid? Kal Ka2 A. 2.1 x 104 8.9 x 10-5 В. 3.2 х 10-6 2.2 x 10-10 С. 4.5 х 10-10 6.7 x 10-6 D. 5.3 x 10-5 1.8 x 10-4