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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:An analytical chemist weighs out 0.099g of an unknown
monoprotic acid into a 250mL volumetric flask and
dilutes to the mark with distilled water. She then titrates
this solution with 0.1800M NaOH solution. When the
titration reaches the equivalence point, the chemist
finds she has added 10.5mL of NaOH solution.
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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 garrow_forwardA 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/unitsarrow_forward2. 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%)arrow_forward
- 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.arrow_forwardA 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.arrow_forwardYou 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?arrow_forward
- helparrow_forwardA 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 %3Darrow_forwardA 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.arrow_forward
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