o A 55.0 mL solution of 0.150 M potassium alaninate ( H₂NC₂H₂CO₂K) is titrated with 0.150 M HCl. The pKa values for the amino acid alanine are 2.344 (pKal) and 9.868 (pK₂2), which correspond to the carboxylic acid and amino groups, respectively. Calculate the pH at the first equivalence point. pH = Calculate the pH at the second equivalence point. pH = H₂N- CH3 -CH- K Potassium Alaninate

An analytical chemist is titrating 152.0 mL of a 0.2100 M solution of benzoic acid (HCH,CO,) with a 0.6700 M solution of NaOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 29.70 mL of the NaOH solution to it.

An analytical chemist is titrating 64.9 mL of a 0.5800M solution of isopropylamine ((CH3),CHNH2) with a 0.3400M solution of HNO3. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 69.8 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,3 solution added. Round your answer to 2 decimal places. pH =

An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ||

An analytical chemist is titrating 111.5 mL of a 0.2600M solution of acetic acid (HCH,CO,) with a 0.5100M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 10.45 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = |

Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Based on the information provided, set up a RICE/ICE Table to answer the question. Let x represent the original concentration of CH₃COOH in the water.

in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.

A chemist titrates 100.0 mL of a 0.5181 M carbonic acid (H,CO, solution with 0.7276 M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K, of carbonic acid is 3.60. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added.

Calculating the pH at equivalence of a titration A chemist titrates 170.0 mL of a 0.2614M cyanic acid (HCNO) solution with 0.7980M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K, of cyanic acid is 3.46. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added. pH =

In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a)  Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b)  Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c)  Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.