Calculating the pH at equivalence of a titration A chemist titrates 250.0 mL of a 0.5755 M nitrous acid (HNO,) solution with 0.0749 M NaOH solution at 25 °C. Calculate the pH at equivalence. The pK, of nitrous acid is 3.35. 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 = ||

A chemist titrates 60.0 mL of a 0.2562M benzoic acid (HC6H5CO₂) solution with 0.0811M KOH solution at 25 °C. Calculate the pH at equivalence. The pK of benzoic acid is 4.20. a 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 KOH solution added. pH = X S

A chemistry graduate student is given 100. mL of a 0.40M nitrous acid (HNO,) solution. Nitrous acid is a weak acid with K 4.5 x 10. What mass of -4 NaNO, should the student dissolve in the HNO, solution to turn it into a buffer with pH =3.16? %3D You may assume that the volume of the solution doesn't change when the NaNO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10 Submit Assignment Continue 2021 McGraw Hill LLC. AlI Rights Reserved. Terms of Use Privacy Center | Accessibility MacBook Air F11 Fig

Question 7

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.

Calculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.5851 M ethylamine (C2H5NH2) solution with 0.8192M HBr solution at 25 °C. Calculate the pH at equivalence. The pK of ethylamine is 3.19. b 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 HBr solution added. pH = ] ☑

A chemist titrates 160.0 mL of a 0.6712M benzoic acid (HC6H5CO₂) solution with 0.6137M NaOH solution at 25 °C. Calculate the pH at equivalence. The pk of benzoic acid is 4.20. a 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 = X

A 27.0 mL solution of 0.110 M CH3COOH is titrated with a 0.210 M KOH solution. Calculate the pH after the following additions of the KOH solution: Note: Reference the K of acids at 25 °C table for additional information. a Part 1 of 2 0.00 mL KOH added. Be sure your answer has the correct number of significant digits. pH ==== 2.85 Part 2 of 2 5.00 mL KOH added. Be sure your answer has the correct number of significant digits. Check pH = => 4.48 X Save For Later Submit Assignment

A 20.00-mL sample contains 1.00 g of NAHCO,. This sample is used to standardize an NaOH solution. At the equivalence point, 39.60 mL of NaÓH have been added. K,(HCO, ) = 4.8 x 10 Indicators that change color within the pH range: bromothymol blue = 6.0 – 7.7 phenolphthalein = 8.3 – 9.8 alizarin yellow R = 10.0 – 12.0 a. What was the concentration of the NaOH? Concentration M b. What is the pH at the equivalence point? pH = c. Which indicator, bromothymol blue, phenolphthalein, or alizarin yellow R, should be used in the titration? bromothymol blue phenolphthalein allzarin yellow R y Another Version 10 item attempts remaining

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 10 20 30 40 50 60 70 80 90 Volume of HCl added (ml) Possible identities for the three liquid bases are shown in the table below. Base pyrole pyrimidine pyridine triethylamine 2.51 x 10-14 1.25 x 10-13 1.70 x 10-9 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter. Hd