2. Should the molarity of the base change when titrating? Explain. 3. a. Write the acid base equation for hydrochloric acid reacting with calcium hydroxide. b. If 40.0 mL of 0.250 M calcium hydroxide is needed to reach the endpoint of 10.0 ml of a hydrochloric acid solution. What is the molarity of the hydrochloric acid solution? 4. What would or would not happen if no phenolphthalein was added to the solution?

A 2.500-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.00 mL of 0.798 M HCl. Some acid remains after the treatment of the sample. a Write the net ionic equation for the complete reaction of sodium carbonate with hydrochloric acid b If 28.7 mL of 0.108 M NaOH were required to titrate the excess hydrochloric acid, how many moles of sodium carbonate were present in the original sample? c What is the percent composition of the original sample?

Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.

You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.

Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.

Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.

QUESTION 4 Standardizing a solution of sodium hydroxide for our acid-base titration experiment means O a. to prepare a series of standard solutions and determine the average concentration. O b.to prepare the standard solution directly from a solid and not from a solution. O c. to compare the results of your titration with those of other laboratories, or other groups performing the same titration. O d. to determine, by titration , the concentration of the basic solution using a known quantity of a primary standard acid. Click Save and Submit to save and submit. Click Save All Answers to save all answers. F7 F8 F9 F10 F11 F12 Inse

7) What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration .

moles of NaOH moles moles of acid moles Concentration of acid in original sample in M Volume in mL

2. If 25 ml of HCl solution required 26.25 ml of 0.0952N sodium hydroxide in a titration, what volume of the solution would produce 0.2867g of AgCl? (determine the N of acid solution, then use it for the volume that will react with AgCl)