A 1.00 M solution of fluoroacetic acid is 10.0 % dissociated in water at a certain temperature. a. What is the pOH of the solution? b. What will be the corresponding dissociation constant for the acid? c. What will be the expected new pH if the solution is diluted to 1.00 x 10*?

1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid  has a pKa of 8.27.  Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE

Calculate the pH of each of the following solutions   a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5   b. 0.10 M sodium propanoate, NaCH3CH2COO.   c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate   d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate   e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate

19. A student prepared a 250.0 mL solution by dissolving 4.559 g of (NH4)2SO4 in enough water. The temperature is 298 K. The base dissociation constant for NH3 is 1.796x10-5. Please answer the following questions. A. B. What is the equilibrium concentration of H3O+ in the solution? Please provider your answer below. 00 + → What is the equilibrium concentration of OH in the solution? Please provider your answer below. OO → $ → $ C. What is the pH of the solution? pH = Please provider your answer below. S M M

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

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18.   A. Calculate [OH−] for this strong base solution: 7.3×10−2 M KOH and then it's pH   B. Calculate [OH−] for this strong base solution: 10.0 mL of 1.00×10−2 M Ca(OH)2 diluted to 500.0 mL and it's pH   C. Calculate [OH−] for the strong base solution formed by mixing 10.0 mL of 1.50×10−2 M Ba(OH)2 with 34.0 mL of 6.0×10−3 M NaOH and it's pH

1. Acetic acid is a weak monoprotic acid with Ka = 1.77 x 10¯5. NaOH(s) was gradually added to 1.00 L of 0.0179 M acetic acid. (Assume no volume change occurs.) Calculate the pH of the solution after the addition of 0.0286 mol of NaOH(s).    A.  8.502  B.  1.971  C.  12.029  D.  7.000 2.What is the ratio of [A-] / [HA] for a buffer solution of HA with a pH of 7 if the pKa = 5 for HA?      A.  100  B.  0.01  C.  10  D.  0.1 3.  Titrate 50.0 ml 0.1 M HCN (Ka = 6.2 x 10-10) with 0.10 M NaOH. Calculate the pH at the half-way or midpoint.    A.  9.2  B.  7.0  C.  4.8  D.  0.0