A 7.00 mL aliquote of acetic acid was mixed with water and the resulting solution was titrated with 0.250 M NaOH. It took 40.2 mL of base to reach the equivalence point. What was the concentration of the acetic acid?
1) 0.043 M
2) 0.070 M
3) 0.143 M
4) 1.43 M
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
A 7.00 mL aliquote of acetic acid was mixed with water and the resulting solution was...
1) Acetic Acid is mixed with water in an experiment. The resulting concentration of H3O+ ions in the reaction at equilibrium (after everything has been mixed) is 0.013M. What is the pH of the new solution at equilibrium? 2) A neutralization reaction with Acetic Acid and Sodium Hydroxide is run: CH3COOH + NaOH -> CH3COONa + H2O When the conjugate base (CH3COONa) concentration is 0.008M and the conjugate acid (CH3COOH) concentration in 0.0032M, what is the pH of the solution?...
Calculate the pH of a 25.0 mL of 0.100M base acetic acid solution after being titrated with 0.100 M NaOH to its equivalence point (pKb (acetic acid)=5.68x10^-10)
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
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
please show all work. thank you
A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02), is titrated with 0.5003 M NaOH, and 15.00 mL is required to reach the a. What is the molarity of the acetic acid? b. If the density of the vinegar is 1.006 g/cm3, what is the mass percent of acetic acid in the vinegar?
A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02),...
32.65 mL of a solution of the acid H2C2O4 is titrated, and 43.90 mL of 0.7300-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.
42.04 mL of a solution of the acid HNO3 is titrated, and 52.40 mL of 0.5500-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.
Trial 1 Acetic acid / L solution 2.402g/L Volume of acetic acid (mL) 30 mL Initial buret volume (mL) 0.2 mL Final buret volume at end point (mL) 18.2 mL Total volume of NaOH titrated (mol) 18.0 mL Moles of NaOH titrated (mol) Molarity of acetic acid (mol/L) Molar mass of acetic acid Average volume of NaOH titrated mL Average molar concentration of acid Average molar mass of acetic acid
26.24 mL of a solution of the acid H2C2O4 is titrated, and 84.20 mL of 0.4200-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution. How many M?