We are titrating 20.0 mL of 0.100 M NaOH(strong base) with 0.250 M HCl(strong acid). What is the pH when the following volumes of HCI are added: 0 mL, 2.00 mL, 4.00 mL, 7.00 mL, 8.00 mL, 3. 9.00 mL, 12.00 mL. For each volume, also state the species and the concentrations of the species present right after the base and acid react. (Ans. 0 mL, pH=13.00; 2 mL, pH-12.83; 4 mL, pH-12.62; 7 mL, pH-11.97 8 mL, pH-7; 9 mL, pH-2.06; 12 mL, pH-1.50)

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If the initial volume reading for the first titration was 0.16 mL and the final volume reading was 11.68 mL, what volume of iodine solution was used in your first titration (in mL)? Include the unit in your answer and two decimal places in your answer.

SHOW WORK. Calculate how many mL of 0.0857 M AgNO3 are required to prepare 100.00 mL of a 0.0133 M solution. Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Enter a question mark for the variable being calculated. Be sure to identify terms for the original solution as M, and V1, and terms for the final solution as M2 and V2. Do not leave any blank empty. M1 = V1= M2 = V2= Rearrange the dilution equation carefully needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Use the following abbreviations: original (or stock solution) molarity M1, volume of original solution = V1, final molarity of new solution = M2, final volume of new solution = V2 Terms in the numerator: Terms in the…