47. Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the vol- ume of each unknown HCl solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Calculate the con- centration (in M) of the unknown HCl solution in each case. HCI Volume (mL) NaOH Volume (mL) [NaOH] (M) 0.1231 M 0.0972 M 0.1178 M 0.1325 M a. 25.00 mL b. 15.00 mL c. 20.00 mL d. 5.00 mL 28.44 mL 21.22 mL 14.88 mL 6.88 mL

The figure below is an example of a titration curve for Terating trprotic acid with a stong base 10 10 20 Velume of bese (m) O a diprotic acid with a strong base. O a triprotic acid with a strong base. a mixture of a strong monoprotic acid and a weak monoprotic acid with a strong base. O a mixture of a strong monoprotic acid and a weak diprotic acid with a strong base. 12

Which of the following is true? a) To lower the pH of an indicator solution, add NaOH. To raise the pH of an indicator solution, add HCI. b) Either HCI or NaOH can be used to raise the pH of an indicator solution. O c) To lower the pH of an indicator solution, add HCI. To raise the pH of an indicator solution, add NaOH. d) Either HCI or NaOH can be used to lower the pH of an indicator solution.

Can someone help with this question. Ten mL of a stock solution of the bromocresol green indicator is mixed with 10 mL of NaOH. Which of the following is true? Select one: a. The concentration of the indicator increases. b. The concentration of the indicator decreases. c. The concentration of the indicator remains the same. d. None of the above.

What is the purpose of a titration? Explain the logic/steps of carrying out a titration, specifying the importance of each step in the process.

A 0.17 M solution of a diprotic acid is titrated to neutralization with 35.1 mL of 0.18 M LiOH. How many mL of the acid are required to reach the equivalence point?

In general, adding a strong acid or a strong base to a buffer solution _________ neutralizes the solution making a solution that is neither acidic nor basic. drastically changes the pH to be either strongly acidic or strongly basic. causes only a slight change in pH making the solution only a little more acidic or only a little more basic than it already was. has variable results so there is no general trend

You are titrating a 25.0 mL HCl sample of unknown molarity. It takes 25.4 mL of 0.100M NaOH to reach the equivalence point. What is the concentration of HCl?

In a titration of 64.0 mL of a 0.500 M solution of a diprotic acid H.C.H.O. (malonic acid) with 0.255 M NaOH, how many mL of base are required to reach the second equivalence point?

A 0.590 g sample of a diprotic acid is dissolved in water and titrated with 0.160 M NaOH. What is the molar mass of the acid if 32.5 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol