2 Determine the mass of solute in 3.60 L of 0.200 M acetic acid, HC,H,O, (FW...
P abanatory we r e to be completed amly your scheduled Laboratory period. POST LABORATORY QUESTIONS 1 Determine the molarity of a solution obtained by dissolving 8.56 KIO, (W 2140) in sufficient water to obtain a 2000. mL of solution Determine the mass of solute in 3.60 L of 0.200 Macetic acid, HC,H,O, (FW-60.0). 3 What is the molarity of a hydrochloric acid sample if 15.0 mL of 1.20 M NaOH are required to neutralize 45.0 mL of the acid?...
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂ after 100.0 mL of the strong base has been added. The value of Ka for HC₄H₇O₂ is 1.5 × 10⁻⁵. HC4H7O2 (aq) + OH- --> H2O (l) +C4H7O2-
OL 20.00 1 C2 =.936 M 45. 7.00 mL of acetic acid is titrated with NaOH. If 19.2 mL of 0.200 M NaOH is nec equivalence point, what is the concentration of the acid? Macid & Vaida Mo NaOH 19.2 mL = .0192 L 7.00mL needed HC 2 H ₃ Oz NaOH Na C2 H₂O2 + H₂O. 200M HC₂ H₂ O2 + NaOH 2oom ,200 ni 290X 7.0 Mb 7.oom you 19 1. f 450 mL is completely neutralized
a) A 50.0 mL solution of 0.200 M acetic acid (CH3COOH), 50.0 mL of 0.200 M is titrated with 0.200 M NaOH. Determine the pH.of acetic acid before any NaOH is added. The Ka of CH3COOH is 1.8 x 10-5. b) Determine the pH of the solution at the equivalent point.
5. Acetic acid (HC,H,Os) is an important component of vinegar. A 10.00-ml sample of vinegar is titrated with 0.5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present a. Write a balanced equation for this neutralization reaction. b. What is the molarity of the acetic acid in this vinegar? c. If the density of the vinegar is 1.006 g/mL, what is the mass percent of acetic acid in the vinegar? 6. How many milliliters...
Calculate the number of grams of solute in 0.250 L of 0.200 m KBr
Part A Calculate the pH of a 0.200 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8x10-5 11.28 O 2.72 O 4.98 O 9.02
A 260.0 mL buffer solution is 0.200 M in acetic acid and 0.200 M in sodium acetate (For all answers express them using two decimal places) A) What is the initial pH of this solution B) What is the pH after addition of 0.0150 mol of HCl C) What is the pH after addition of 0.0150 mol of NaOH
What mass of sodium acetate must be added to 1.00 L of 0.10 M acetic acid (pKa= 4.75) to give a solution with a pH of 4.54? Atomic masses: C 12.01, H 1.01, O 16.00, Na 22.99 Present your answer to 1 decimal place. Choose the appropriate units from the drop down box.
Q. A buffer solution prepared by mixing 50.00 mL of 0.200 M acetic acid and 50.00 mL of 0.200 M sodium acetate (Ka, acetic acid = 1.76 x 10-5). (Hint: Calculate the pH using the Henderson-Hasselbach equation, remember to allow for the dilution effect when mixing the two solutions together.)