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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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You have a 25.00 mL sample of H3PO4 with an unknown concentration. In order to determine the concentration, you set up a titration using 0.500 M KOH. It takes the addition of 9.67 mL of your titration to reach the endpoint. What is the concentration (in M) of H3PO4 in your initial sample?
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- QUESTION 5 Consider the titration of 17.7 mL of 0.211 M HNO3 with 0.130 M NaOH solution. What volume (in L) of NaOH is required to reach the equivalence point in the titration? Give your answer in numerical form (NOT exponential notation) using the correct number of significant figures. Lavide jon.arrow_forwardA 0.478 g sample of an unknown strong base is dissolved in 50.0 mL of water and titrated with a 0.135 M HCL solution. The equivalence point is reached when a total of 29.0 mL of HCL is added. The base and acid conbine in a 1:1 ratio. (a) How many moles of base are neutralized when the equivalent point is reached? (b) What was the initial concentration (M) of this unknown base? (c) What is the molar mass of the unknown base?arrow_forwardTitration of 25.0 mL of an unknown concentration H2SO4 solution requires 37.6 mL of 0.1375 M NaOH solution. What is the concentration of the H2SO4 solution (in M)?arrow_forward
- The titration of a 5.00 mL sample of an HCl solution of unknown concentration requires 4.90 mL of a 0.1000 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M?arrow_forwardAn HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution? 2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution? 3. What is the concentration of Ag+ in solution?arrow_forward10.5 mL of 0.139 M Mg(NO3)2 is mixed with 11.9 mL of 0.625 M NaOH. Calculate the final concentration (in M) of hydroxide ion ([OH-]) after any reaction that occurs goes to completionarrow_forward
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