A chemist makes a new solution: 1.0 L of a solution that is both that is both 0.6 M NH3 and 0.8 M NH,CI. What is the pH of the solution after 0.10 mol of NaOH is added? Round your answer to 2 decimal places. There is no change in volume upon addition of NaOH. pH =

A chemist makes a new solution: 1.0L of a solution that is both that is both 0.6 M NH; and 0.8 M NH,CI. What is the pH of the solution after 0.10 mol of NAOH is added? Round your answer to 2 decimal places. There is no change in volume upon addition of NaOH. pH =

Suppose 90.00 mL of 0.200M HCl is added to an acetate buffer prepared by dissolving 0.100 mol of acetic acid and 0.110 mol of sodium acetate in 0.100 L of solution. What are the initial and final pH values? What would be the pH if the same amount of HCI solution were added to 190 mL of pure water? Initial pH = Final pH pH after HCl is added to water =

During a titration a 0.30 L sample of H2SO4 requires 569 mL of 2.50 M NaOH to reach the equivalence point. What is the initial concentration of H2SO4? (Do not include units in your answer. If you round during your calculation make sure to keep at least 3 decimal places. Report your answer to 2 decimal places.)

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?

A 0.035 M solution of a weak base is 0.022% ionized. What is the pH of the solution? What is the value of Kb for the base? Enter in scientific notation, for example, 0.00010 would be 1.0E-4.

please solve both question. each image has different question.

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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?

Enough water was mixed with 1.26 g of sodium hydroxide (40.0 g/mol) to make a 500. mL solution. What is the pH of this NaOH solution?