1. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid, H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is the concentration of the phosphoric acid solution using the results that were obtained? K Given: H₂PO4(aq) + 3NaOH(aq) - Na3PO4(aq) + 3H₂O(1)

2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium acetate (CH3COONa) together in a beaker: a. The Ka of acetic acid is 1.8 x 105. What is the pH of the solution that you made? What is the degree of ionization? CH&COOH+ CHeCOONat lOH 4 g CH300H

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A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.14 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. During the titration the following reaction occurs      HA + NaOH ⇒ NaA + H2OWhat is the concentration of A- (the conjugate base of the weak acid) at the equivalence point?   ml NaOH added pH Hal-way point 18.71 3.41 Equivalence point 37.41 8.53

Can you help me answer the PH=

100.0 mL of HCI required 25.00 mL of 0.2000 M Mg(OH)2 to reach pH 7. What is the concentration of the HCI ? 2 HCI + Mg(OH)₂ MgCl₂ + 2 H₂O The neutralization equation is There is enough information to calculate the moles of Mg(OH)2 ( L Mg(OH)₂ (- concentration = Then use stoichiometry to convert moles of Mg(OH)₂ into moles of HCI mol HCI a. acid i. 0.2000 p. 0.01000 mol Mg(OH)₂ (- b. base c. HCI d. NaOH mol Mg(OH)2 We now can calculate the concentration of HCI since we have both the moles of HCI and the volume of HCI j. 1.000 k. 0.005000 q. 0.001000 1 L mol HCI LHCI r. 58.31 = mol Mg(OH)2 e. NaCl I. 100.0 f. H₂O m. 0.1000 s. 5.831 = g. 25.00 mol/L n. 0.05000 h. 0.02500 mol Mg(OH)2 o. 2.000 mol HCI

An analytical chemist is titrating 143.6 mL of a 0.7000M solution of piperidine (C,H10NH) with a 0.4000M solution of HNO3. The p K, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 267.7 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

ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 7.00 ✕ 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH-(aq)  C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2-   M Na+  M H3O+  M OH-  M C6H5CO2-

20. mL of 0.250 M NH3 is titrated with 0.500 M of HCl solution, what is the pH of the resulting solution when 0mL, 5.0 mL, 10.0 mL and 12 mL of HCl was added into the NH3solution? KB(NH3) = 1.8 x 10-5

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq)  C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2-   M H3O+  M OH-