A buffer solution is made up of 1.0 M NH3 and 1.0 M NH4CI. KbNH3 = 1.8 × 10-5 x What is the pH when 50 mL of 0.40 M HCI is added to 25. mL of the buffer? pH after acid added pH = Enter

Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7

4. Consider a buffer made by adding 0.050 mol NaC2H302 and 0.040 mol HC2H3O2 to a liter of water. a) What is the pH of this buffer? b) What is the pH after addition of 0.010 mol NaOH? c) What is the pH after addition of 0.010 mol HCI to the original buffer solution?

Calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. For 230.0 mL of a buffer solution that is 0.2604 M in CH3CH2NH2 and 0.2404 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH(Kb=5.6⋅10^−4).

What will be the pH of the final solution if 1.50 x 10-2 mol HCl solution is added to the buffer solution (100 mL) that contains 1.0 M HCN and 1.2 M NaCN?

7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?

A Titration of 10.0 mL of 0.15 M NaOH is added 0.35 M HNO3. What is the volume of HNO3 to reach equivalent  point? 40.0 mL of 0.350 M CH3NH2 is titrated with 0.280 M HCI until the end point is reached. What is the pH of the solution at the end point. (Kb for CH3NH2  = 5.0 X 10^-4)

Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 100.0 mL of the strong base has been added. The value of Ka for HC4H;O2 is 1.5 × 10-5 1 2 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HC4H;O2(aq) + OH (aq) H20(1) + C4H,O2 (aq) Before (mol) |Change Imol) After | (mol) RESET 0.100 0.200 +x 0.100 + x 0.100 - x -x 0.200 + x 0.200 - x 2.00 x 103 -2.00 x 103 8.00 x 103 -8.00 х 10"3 1.00 x 102 -1.00 x 102 1.20 х 10"2 -1.20 x 102 2.00 x 10-2 -2.00 x 102