A chemist prepares a 0.50 M solution of NaF which gives a measured pH of 8.58; and also prepares a 0.50 M solution of NH4Cl which gives a measured pH of 4.78. Write net ionic equations consistent with each of these observations?

Original concentration of Acetic Acid was 0.1033 M and NaOH was 0.1104 M there is part a done, need to do part B

For each of the salts (assume at this point completely soluble), write the equation for dissociation and label the ions as acidic, basic or neutral.Each salt listed will 100% dissociate  NH4C2H3O2 Al2(CO3)3 Na2HPO4 NaI   For each of the following salts, determine the pH of a 2.50M solution of the salt.You will need the Ka and Kb tables to complete this problem.   NaBrO  CH3NH3Cl NaClO2 C6H5OK CsNO3 C6H5NH3Br

a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3?  The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.

What is the pH of the resulting solution when 12.50 mL of 0.45 M HCI is titrated with 17.00 mL of 0.28 M CSOH? Report your answer with the correct number of significant figures.

Please answer these questions on your Page 9 We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.11. We titrate this solution with a 0.166 M NaOH solution and we need 22.2 mL of this NaOH solution to reach the equivalence point. The temperature is 25.0°C throughout. (a) What is the molar mass of HA? (b) What is the dissociation constant, K₁, of A-(aq)? (c) What was the pH of the solution after the addition of the first 15.0 mL of the NaOH solution?

Please answer these questions on your Page 9 We dissolve 1.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution is 1.33. We titrate this solution with a 0.277 M solution of NaOH and we need 14.4 mL of this NaOH solution to reach the equivalence point. The temperature is 25.0°C throughout. (a) ) What is the molar mass of HA? (b) ) What is the dissociation constant, Ka, of HA(aq)? (c) ( What is the pH at the equivalence point?

A solution is prepared by dissolving 15.0 g of pure HC2H3O2 and 25.0 g of NaC2H3O2 in 775 mL of solution (the final volume). (a) What is the pH of the solution? i (b) What would the pH of the solution be if 25.0 mL of 0.250 M NaOH were added? i (c) What would the pH be if 25.0 mL of 0.40 M HCI were added to the original 775 mL of buffer solution?