2. (4 pts) For each [OH-] below, give the [H30+1 a. 10.0 x 10-6 M b....
You must show your work to receive credit. pH = -log[H₂O 1.(4 pts) For each [H3O+] below, give the pH. a. 8.7 x 10-8 M b. 7.9 x 100M 17.06 18. 2. (4 pts) For each [OH-] below, give the [H3O+] a. 10.0 x 10-6 M b. 8.4 x 10-M 1x 10 9 3. (4 pts) For each pH below, give the [H30“). 10 a. 8.5 b. 2.9 ..th 0:1.0*11- Сен 10 P7 13.16 *10-9 11.26 x 10-3 4. (4...
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
Which of the following statements describes a basic solution? 1. [H30+]> [OH] 2. [H30]<[OH] 3. [H30'] x [OH] #1 x 10-14 4. [H3O+]/[OH] = 1 x 10-14 5. [H3O+]/[OH]=1 If the pH of a solution is 10, what is the hydronium, H ion concentration? 1. A) 1 x 10-10 M 2. B) 1 x 1010 M 3. C) 10 M 4. D) 10 M 5.E) * 1 1010 M As the pH increases the hydroxide ion concentration 1. A) goes...
For each strong base solution, determine [OH−], [H3O+], pH, and pOH. 1.0×10−4 M Ca(OH)2, determine [OH−] and [H3O+]. For this solution determine pH and pOH. 2.9×10−4 M KOH, determine [OH−] and [H3O+]. For this solution determine pH and pOH.
please show all work neatly 5. (2 pts) Consider the following acids and their dissociation constants HPO4-2(aq) + H2O.. H3O"(aq) + PO4-3(aq) Ka-2.2x 10.13 HCOOH(aq) H20 H3O (a) HCOO (aq) Ka = 1.8x10-4 a. Which is the weaker acid, HPO42 or HCOOH? b. What is the conjugate base of, HPO42 or c. Which acid has the weaker conjugate base? d. Which acid produces more ions? 6. (2 pts) Write a balanced equation for the neutralization of H3PO4(aq) and NaOH(aq) (3...
2. A buffer is prepared by partially titrating 50.00 mL of 0.964 M benzoic acid using 0.100 M NaOH until the pH is 4.80. Ka for benzoic acid is 6.3 x 10-5. (o)ce pts) What ratio of the conjugaite base-to-conjugate acid i equrd to establish p 4 (b) (1 pts) What volume of the titrant is required to achieve pH 4.80? (c) (2 pts) What are the final concentrations of the conjugate acid and conjugate base? 2. A buffer is...
For each strong acid solutions, determine [H3O+],[OH−], and pH. 1. 0.21 M HCl. 2. 2.6×10-2 M HNO3 3. a solution that is 5.1×10−2 M in HBr and 1.7×10−2 M in HNO3 4. a solution that is 0.675 % HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)
For each strong acid solutions, determine [H3O+],[OH−], and pH. 1. a solution that is 6.8×10−2 M in HBr and 2.4×10−2 M in HNO3 2. a solution that is 0.610 % HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)
Calculate the pH of each of the following solutions. (a) 1.3 x 10-4 M Ba(OH)2: x 10 (Enter your answer in scientific notation.) (b) 1.7 x 10-4 M HNO3: Calculate the pH of a 0.025 M CHEN (pyridine) solution. The K, for pyridine is 1.7 x 10 9. pH =
Problem Set 15 CHEM 1252 November 10, 2019 4. A 0.100 M solution of bromoacetic acid (BrCH COH) is 13.2% Ionized dissociated). (a) Calculate [H3O+] (or "[*]"), [BrCH.CO." ] (or "[A-]"), and (BrCH2COH) (or "CHA]"). (b) Calculate K, and pk, for bromoacetic acid. 5. Ethylamine (CHCH NH) is a weak base in water. (a) Write a balanced chemical equilibrium reaction for the base hydrolysis of ethylamine. Label the acid, base, conjugate acid, and conjugate base. (b) Would you expect ethylammonium...