Calculate the moles of KHP titrated in each trial = M x L = 0.5 M x 0.025 L=Calculate the moles of NaOH using stoichiometry of the reaction Table 1.1st Trial2nd Trial3rd Trial4th TrialInitial Burette reading(ml)2.015.12.015.0Final Burette reading(ml)15.128.115.028.1Volume of NaOH delivered in ml13.113.013.013.1L of NaOH delivered0.01310.01300.01300.0131Table 2.1st Trial2nd Trial3rd Trial4th TrialMolarity of NaOH0.954 M0.962M0.962 M0.954 MAverage molarity0.958 M

KHP or potassium hydrogen phthalate is a monobasic acid. It is used as primary standard to…

Answered: Calculate the moles of KHP titrated in…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.98QE

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Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If 19.45 mL NaOH is required to neutralize 0.442 g KHP, what is the concentration of the NaOH?
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction?
Q7. Karl Fisher titration is used to determine moisture content of food products according to the chemical reaction below: 2H₂O + SO₂ + 12 → H₂SO4 + 2HI (i) Name the reaction that involved. (ii) Identify the FOUR major chemical components needed in the Karl Fisher reagents. (iii) Rewrite the actual chemical reaction(s) that involved during Karl Fisher titration. (iv) Outline the function of each major chemicals in the reaction stated in answer (iii).
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2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
D. Acid-Base Titrations A 0.1558 g of primary-standard-grade benzoic acid, C6H$COOH, was used to standardize a solution of Mg(OH)2. Calculate the normality of this solution if it needed 19.15 mL of this base to reach the end point of the titration. A solution of an unknown monoprotic acid was found in a laboratory. When titrated, 25.00 mL of this unknown solution needed 28.44 mL of the same base to reach the endpoint. The remaining solution of unknown monoprotic acid amounting 15.00 mL was left in an Erlenmeyer flask uncovered to recover the acid crystals. After 5 days, the mass of the unknown monoprotic acid left on the flask weighed 0.0967 g. Determine the equivalent weight of this unknown acid. FW: C6HSCOOH: 122.12 Mg(OH)2 = 58.32
Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titrations. If 20.35 ml. NaOH is required to neutralize 0.472 g KHP, what is the concentration of the NaOH? concentration:
A titration is used to determine the concentration of a specific substance in solution. O True O False

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Calculate the moles of KHP titrated in each trial = M xL = 0.5 M x 0.025 L=_ Calculate the moles of NaOH using stoichiometry of the reaction