3. What is the concentration of a NaOH solution if it reacts with O.6008 g of KHC8H4O4 and the equivalence point is reached after 18.53 mL of base has been added? The reaction is given by KHC &H4O4 (s) +NaOH (aq) KNaC8H4O4 (aq)+ H20 () 13

What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.

When a 22.9 mL sample of a 0.351 M aqueous acetic acid solution is titrated with a 0.445 M aqueous potassium hydroxide solution, what is the pH after 27.1 mL of potassium hydroxide have been added? pH =

How many equivalents are in 15.0 mL of 0.12 M Ba(OH)2 solution? What volume of 0.085 M HNO3 is required to reach the end point when titrating 15.0 mL of this solution?

10.5 mL of 0.139 M Mg(NO3)2 is mixed with 11.9 mL of 0.625 M NaOH. Calculate the final concentration (in M) of hydroxide ion ([OH-]) after any reaction that occurs goes to completion

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO₂H, in enough water to make 1.00 x 102 mL of solution and then titrate the solution with 0.133 M NaOH. C6H5CO₂H(aq) + OH(aq) C6H5CO₂ (aq) + H₂O(f) What are the concentrations of the following ions at the equivalence point? Na+, H₂O+, OH C6H5CO₂ 0.0168 ✓ M Na+ 1.82e-8 M H3O+ 5.45e-7 × MOH 0.0168 M C6H5CO₂ What is the pH of the solution? 7.74

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

7.  The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq)                      (Z) 25.0 mL of 1.0 M CH3COOH(aq)   Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True

What volume, mL, of a 0.121M NaOH solution is required to reach the endpoint in a complete titration of a 10.0 mL sample of 0.102 M H2SO4? H2SO4 (aq) +      NaOH (aq) →     H2O (l) +    Na2SO4 (aq)

42. A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions:   Volume of CH3COOH(aq):   139.0 mL Concentration of CH3COOH(aq):  1.103 M   Volume of CH3COONa(aq):  127.0 mL Concentration of CH3COONa(aq):  1.259 M   Calculate the pH of this buffer after the addition of 20.00 mL of 3.00 M sodium hydroxide, NaOH, a strong base.     4.38     5.90     4.69     4.81     5.12