An analytical chemist weighs out 0.099g of an unknownmonoprotic acid into a 250mL volumetric flask anddilutes to the mark with distilled water. She then titratesthis solution with 0.1800M NaOH solution. When thetitration reaches the equivalence point, the chemistfinds she has added 10.5mL of NaOH solution.

Given,molarity of NaOH = 0.1800 mol/Lvolume of NaOH = 10.5 mL number of moles of NaOH can be…

Answered: An analytical chemist weighs out 0.099g…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
A 5.50 mL sample of an H3PO4H3PO4 solution of unknown concentration is titrated with a 1.050×10−2 MNaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4H3PO4 solution? Express your answer with the appropriate units. value/units
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%)
You have three flasks with 0.03 M chloride, bromide & iodide ions. If you titrated a mixture containing the three ions with silver nitrate, what order will the equivalence points appear in the titration curve? Ksp AgCl = 1.8 x 10^-10 Ksp AgBr = 5.0x10^-13 Ksp Agl = 8.3 x 10^-17
40 mL of LiOH are titrated to the equivalence point with 65 mL of 1.2 x 10-2 M HNO3. Find the concentration (molarity) of the LiOH solution.
Which of the following statements is/are TRUE when the purity of the KHP is not considered in the calculation of the molarity of the 0.10M NaOH titrant?I. The calculated concentration of the acetic acid would be less than the true concentration of the acetic acid in the vinegar sample.II. The volume of the 0.1M NaOH titrant that would be used in titrating the soda samples would be lower than the supposedly titrant volume to reach the endpoint.III. The calculated concentration of the acetic acid would be higher than the true concentration of the acetic acid in the vinegar sample. a.I only b.II and III c.III only d.I and II
A 28.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1422 MM KOHKOH solution. A volume of 43.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution? Express your answer using four significant figures.
You are given a solution of HCOOHHCOOH (formic acid) with an approximate concentration of 0.20 MM and you will titrate this with a 0.1105 MM NaOHNaOH. You add 20.00 mLmL of HCOOHHCOOH to the beaker before titrating, and it requires 35.43 mLmL of NaOHNaOH to reach the end point. What is the concentration of the HCOOHHCOOH solution?
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A 25.0 mL volume of HCl solution of unknown concentration is titrated with a 0.124 M NaOH solution. Neutralization of the HCl solution requires 42.1 mL of the NaOH solution. Calculate the concentration of the HCl solution. [HC1] = M %3D
A 0.0750 g sample of an unknown weak monoprotic acid (HA) was dissolved in 25.0 mLof water and titrated with an aqueous solution of 0.0125 M Ca(OH)2. The volume of Ca(OH)2 requiredto bring the solution to the equivalence point was 24.5 mL. Calculate the molar mass of the acid.

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