7. If H,PO, has K, -6.83 x 10, and Hco, has K,-5.8x 10", which is the...
7. If H.PO, has K. = 6.83 x 10", and H.CO, has K, - 5.8 * your answer and explain how you know. (ip) has K. = 5.8 x 10, which is the weaker acid? Circle 8. For a solution with pH = 9.74. calculate the following: (3pts) [H] = [OH'] = pOH =
3. Calculate and insert the proper values to complete the following table: 8pts) [H+M pH Acidic or Basic [OH-M Solution 8.21 POH 1.78 x 10 3.70 x 10-2 4. Give definitions of an Arrhenius acid, a Bronsted-Lowry acid, and a Lewis acid. (3pts) 5. Write the two reactions for the complete dissociation of H.SO., a polyprotic acid. 2pts) 6. Calculate the pH of a 0.015 M solution of HBr. Circle your answer. (2pts)
please help with numbers 7, 8 and 9 showing work 7. If H.PO, has K. -6.83 x 10', and H.CO, has K, -5.8 x 10", which is the weaker acid? Circle your answer and explain how you know. (pt) 8. For a solution with pH = 9.74, calculate the following: 3ps) [OH) = pOH - 9. (pes total) a. A solution of a weak acid with concentration - 0.11 M. is 8.8 % ionized. Calculate its K, value b. Calculate...
3. Calculate and insert the proper values to complete the following table: (818) pH pOH [H+] M [OH-] M Acidic or Basic Solution 8.21 5.79 1.78 x 10 3.70 x 10-2 4. Give definitions of an Arrhenius acid, a Bronsted-Lowry acid, and a Lewis acid. (3pts)
5 & 6 1014 3.70xie - 2.7 5. Write the two reactions for the complete dissociation of H2SO4, a polyprotic acid. (2pts) ph 14- ? 6. Calculate the pH of a 0.015 M solution of HBr. Circle your answer. (2pts) рон pon
please help 3. Calculate and insert the proper values to complete the following table: (8pts) РОН [ОН-] М Acidic or Basic (H+J M PH Solution 8.21 5.79 1.78 x 10 3.70 x 10
Calculate the (OH) and the pH of a solution with an (H+] = 3.2 x 10-" Mat 25 °C. [OH-] = pH = Calculate the (H+) and the pH of a solution with an (OH) = 7.0 x 10 M at 25 °C. M [H*] pH Calculate the (H+) and the [OH-] of a solution with a pH = 8.56 at 25 °C. M M (он) Calculate either [H2O+] or [OH-] for each of the solutions. Solution A: [OH-] =...
Calculate the (H+) and pH of a 2.37 x 10-4 M iodoacetic acid solution. The K, of iodoacetic acid is 6.68 x 10-5. [H+) = M pH =
Calculate the [H+) and pH of a 3.75 x 10-4 M butanoic acid solution. The K, of butanoic acid is 1.52 x 10-5. M pH =
Calculate the [H+] and pH of a 1.23 x 10-4 M nitrous acid solution. The K, of nitrous acid is 7.10 x 10-5. [H+] = 1.4 X10-4 pH = 3.9