25.0 O 0.0600 O 0.240 A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about mol/L. O 0.115 pH of solution in flask O 0.300 12.0 10.0 8.0 6.0 4.0 2.0 Equivalence Point 5 10 15 20 25 30 35 40 45 mL of 0.115 M NaOH added to flask

A student titrates 10.0 mL of 2.0 M formic acid, HCO,H (K.= 1.8 x 10-4), using 1.0 M sodium hydroxide, NaOH. 1. What volume of NaOH solution would be needed to reach the equivalence point? a. 10.0 mL b. 20.0 mL c. 30.0 mL d. 40.0 mL

12.0 10.0 8.0 A pH 6.0 4.0 2.0 0.0 C 0 5 10 15 20 25 30 mL of 0.1 M NaOH The graph above shows the titration curves of four monoprotic acids of varying strengths. All of the acids start out at 0.1 M concentration and 25.0 mL volume. Choose all of the correct statements about these titration curves from the choices below. The titration curve labelled "D" is generated by the strongest acid in the series. In the curves shown above the stronger the acid the less NaOH required for neutralization. The stronger the acid the more important is the pKa of the Indicator used for titration. The Ka of the acid which generates curve "C" is about 103 The weaker the acid the lower the pH of the neutralization point. The acid which generates curve "D" has the highest neutralization-point pH in the series.

O ACIDS AND BASES Calculating the pH of a weak base titrated with a strong acid with a 0.3000 M solution of HNO,. The p K, of An analytical chemist is titrating 160.2 mL of a 0.5000 M solution of dimethylamine ((CH₂)2NH) w dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 280.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places... PH-0 X

Please don't provide handwriting solutions....

The pKa of hypochlorous acid is 7.530. A 51.0 mL solution of 0.122 M sodium hypochlorite (NaOCI) is titrated with 0.323 M HCI. Calculate the pH of the solution after the addition of 7.44 mL of 0.323 M HCl. pH = Calculate the pH of the solution after the addition of 20.0 mL of 0.323 M HCl. pH = 7.73 pH = 2.475 Calculate the pH of the solution at the equivalence point with 0.323 M HCI. & TOOLS

A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka’s for KHP are 1.12 x 10-3 and 3.90 x 10-6   Calculate the pH of this solution before adding any NaOH. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? Calculate the pH of the solution after 100. ml of NaOH have been added.