It requires less volume of NaOH for titration of acetic acid as compared to HCl as HCl is a strong acid which dissociates completely whereas acetic acid is a weak acid which won't dissociate completely. So H+ ion concentration in case of acetic acid will be less than that of H+ ion concentration of HCl . So less volume of NaOH solution is needed.
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IUS. A 21.54-mL volume of 0.130 M NaOH is required to reach the stoichiometric point for...
A 21.54 mL volume of 0.130 M NaOH is required to reach the stoichiometric point for the titration of 25.00 mL of a 0.112 M HCl solution. Would the titration of 25.00mL of a 0.112 M CH3COOH solution require more, less, or the same volume of the 0.130 M NaOH solution? Explain.
43. To reach the stoichiometric point in the titration of 25.0 mL of a 0.200 M aqueous solution of HCl, the addition of 20.0 mL of a 0.250 M aqueous solution of NaOH is required. If an additional 1.0 mL of the titrant is added, what is the pH of the analyte solution at this point? A. 11.98 B. 2.26 C. 11.74 D. 13.40 E. 10.40
What volume in milliliters of a 0.141 M NaOH solution is required to reach the equivalence point in the complete titration of a 14.0 mL sample of 0.112 M H2SO4?
3. What volume of 0.025 M NaOH will be required to reach the endpoint in a titration with 25.00 ml of 0.10 M HCI? Show your work with units and correct significant figures. Circle your answer. 4. Calculate the molarity of a sodium hydroxide solution if 25.00 mL 0.100 M maleic acid requires 22.10 ml of NaOH to reach the endpoint. Show your work with units and correct significant figures. Circle your answer. 5. The following data were collected in...
1. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 2. How many liters of 1.75 M HCl will be required to reach the equivalence point with 1.25 L of 2.5 M KOH 3. Titration reveals that 11.6 mL of 3.0 M sulfuric acid is required to neutralize the sodium hydroxide in 25.00 mL of NaOH solution. What is the molarity of the NaOH solution? 4. Titration...
What volume in milliliters of a 0.141 M NaOH solution is required to reach the equivalence point in the complete titration of a 10.0 ml sample of 0.122 M H2SO4?
Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH analyte. How many mL of NaOH is required to reach the equivalence point? Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH analyte. What will the initial pH of the analyte be if 0.00 mL of NaOH is added?
Consider the titration of a 21.0 −mL sample of 0.105 M HC2H3O2 with 0.130 M NaOH. Determine each of the following. . a. The initial pH b. The volume of added base required to reach the equivalence point c. The pH at 5 mL of added base d. The pH at one-half the equivalence point e. The pH at the equivalence point
a volume of 34.0 mL of 0.100 M KOH was required to reach the endpoint in the titration of a 10.0 mL solution of CH3COOH(pKa= 4.74). Find the initial pH of the CH3COOH solution.( a)0.61 b)1.61 (c)2.61 (d)3.61 (e)4.61
Find the pH of the equivalence point and the volume (mL) of 0.0372 M NaOH needed to reach the equivalence point in the titration of 42.2 mL of 0.0520 M CH3COOH. (K_a of CH_3COOH = 1.8 times 10^-5)