If a weak acid has a pKa value of 5.78, what is the value of Ka for the acid?

A student begins a titration experiment by filling her first buret with unknown acid to the 1.12 mL level.  She fills her second buret with base, NaOH, and records an initial volume of 0.08 mL.  At the end of the titration experiment and after the pale pink endpoint is obtained, she records her final volume of acid in the buret as 18.85 mL, and the final volume of base in the second buret as 28.74 mL.  In the first blank below, please indicate the volume of acid used in her experiment.  In the second blank, please indicate the volume of base used.  For both answers, please report your answer WITH the correct number of significant figures or decimal places, and WITHOUT a unit.    Question 1 options: ___________ answer #1   ___________answer #2

On their third titration trial, the CHM 111 student used 18.80 mL of 0.205 M NaOH(aq) to neutralize 25.0 mL of HCl(aq). Calculate the molar concentration of the HCl solution to the correct number of significant figures.

If the initial volume reading for the first titration was 0.16 mL and the final volume reading was 11.68 mL, what volume of iodine solution was used in your first titration (in mL)? Include the unit in your answer and two decimal places in your answer.

K2SO4 (aq) + 2 H20 () 3. For which reaction will AH and AE be exactly equal to each other? 2 (g) →3 CO2 (g) + 3 H2O (g) B) 2 KOH (aq) + H2SO4 (aq) → K2SO4 (aq) + 2 H2O (1) A) C3H60 (1) +4 02 || C) N2 (g) + O2 (g) → 2 NO (2) + 02 D) 2 H2 (g) + O2 (g) →2 H20 (g) (8) E) None of the above + 02 24.02 + 4.04

Suppose a 0.031M aqueous solution of sulfuric acid (H₂SO4) is prepared. Calculate the equilibrium molarity of SO4. You'll find information on the properties of sulfuric acid in the ALEKS Data resource. Round your answer to 2 significant digits. IM S P X

7B.

1 A solution of 2.50 M formic acid is 0.915% ionized. What is the pH of this solution? Enter your answer, rounded to the correct number of significant figures, in the box. pH = X 2.54 A solution of HA, a weak acid (pKa = 8.112), has a pH = 5.770. [HA]eq = 3.12 x 10-4 M. What was the initial concentration of the weak acid solution? Enter your answer, rounded to the correct number of significant figures, into the box below. If your answer is a decimal, put a O before the decimal point. Do not use scientific notation. pH = 1 [weak acid] initially = X X 4.00 0.00404 An aqueous solution of 0.045 M HA (pKa = 11.11) is prepared. What is the pH of this solution? Enter your answer, rounded to the correct number of significant figures, in box below. If your answer is a decimal, put a 0 before the decimal point. Do not use scientific notation. M 1050301 the

Calculate the volume of a 1.420 M NaOH solution required to titrate 43.15 mL of a 1.500 M H₂PO4 solution. Round your answer to 4 significant digits. mL ☐ x10 X

Balance the following equation by filling the gaps with appropriate numbers. OHg + OHCI + OHg, + OH2