A buffer solution is made that is 0.406 M in HNO2 and 0.406 M in NaNO2. -4 If Ka for HNO2 is 4.50 × 10¬, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.093 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +

A buffer solution is made that is 0.337 M in H₂S and 0.337 M in KHS. If Kal for H₂S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.075 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) + +

A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water.  This solution is titrated with a standardized 0.01252 M HCl solution.  The equivalence point is observed after 17.94 mL of the HCl solution has been added. Use this data to answer the questions below. Calculate the moles of OH-  in the 10.00ml sample. (Hint, moles of OH- at the equivalence point = moles HCl) Your answer should have 4 sig figs. Enter answers in scientific notation

You dissolve 0.194 g of NaOH in 2.00 L of a buffer solution that has [H2PO4] = |HPO, | = 0.188 M. What is the pH of the solution before adding NaOH? (K, for dihydrogen phosphate ion is 6.2 x 10-8.) pH = What is the pH of the solution after adding NaOH? pH =

A buffer solution is made that is 0.402 M in HF and 0.402 M in KF. If Ka for HF is 7.20 x 10-4 what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.107 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3OT instead of H+) + > +

You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?

A buffer solution contains 0.405 M NaHSO3 and 0.332 M Na,SO3. If 0.0248 moles of potassium hydroxide are added to 150. mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding potassium hydroxide) pH =

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

What is the [H3O+] and the pH of a buffer that consists of 0.29 M HNO2 and 0.77 M KNO2? (Ka of HNO2 = 7.1 * 10−4)

A buffer solution is prepared by dissolving 0.10 mol of acetic acid and 0.10 mol of sodium acetate in 1 L of solution. A 10-mL portion of 1 M HCl is then added to the solution. How much does the addition change the pH of the buffer? [Ka (CH3COOH) = 1.8 x 10-5]