(5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) 0.0958 M O 0.383 M O 0.767 M O 0.192 M

(5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) 0.0958 M O 0.383 M O 0.767 M O 0.192 M

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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(3) 11. In a titration it is found that 97.7 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of a solution of HCl(aq). Calculate the concentration of the HCl solution. Show your work. [Hint: Write a balanced equation for the reaction first.]
7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s)  Sr2 (aq)  2F  (aq) 2
7) (30) For questions a- c, you must use dimensional analysis to solve the problems related to the following balanced chemical equation: Vbalanced 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) 22 12 22 a) How many liters of 0.15 M KCl solution are needed to completely react with 13.43 L of 0.175 M lead nitrate solution? b) How many grams of precipitate will form upon mixing the two solutions? c) How many moles of chlorine atoms are present in the amount of precipitate produced?
5:15 1 ull 4G Discussion Assignment #6 O o o INFO DISCUSSION Discussion Assignment #6 Due:Wednesday, 14 Oct 2020, 3:00 PM In titration, one solution is added to another solution until a chemical reaction between the components in the solutions has run to completion. The solution being added is called the titrant, and we say that it solution. The completion of the reaction is usually shown by a change of color caused by a substance called an indicator. used titrate the other A typical titration proceeds in the following way. A specific volume of the solution to be titrated is poured into an Erlenmeyer flask. For example, 15.0 mL of a sulfuric acid solution of unknown concentration is added to a 250 mL Erlenmeyer flask. An indicator is then added to the flask, which changes color when the reaction is complete. The titrant in this example is potassium hydroxide, having a concentration of 0.121 M. The titrant is added to a buret. After slowly adding the titrant to the flask, the reaction…
4.30 A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass. (a) What mass (g) of HNO3 is present per liter of solution? (b) What is the molarity of the solution? M.80.010 8.S (0)
6.6 When a 0.3885 M HCI solution is used to titrate 6.7 ml of a borate solution, the initial volume on the burette is 0.82 ml and the final volume is 18.15 ml. What is the molarity of this borate solution? (This data will be used in the next question.) (Give 4 digits of the calculator answer) O a. 0.01258 M O b. 0.5024 M O c. 0.08426 M O d. none of these O e. 1.452 M O f. 1.005 M Og. 0.001005 M Given the molarity of Borate in question 6.7, what is the value of Ksp from this solution? (Give 4 digits of the calculator answer) (This answer will be needed in the next question). 9--OL X Ob. none of these O c. 12.25 O e. 4.060 Og. 0.5074 6.8 Given the value of Ken from this solution in the previous question, what is MacBook Air
Indicate the concentration of each ion present in the solution formed by mixing the following. Assume that the volumes are additive. Enter your answers, separated by a comma, using three significant figures. (1.) 42.0 mL of 0.140 M NaOH and 37.6 mL of 0.430 M NaOH. (2.) 44.0 mL of 0.150 M Na2SO4 and 25.0 mL of 0.200 M KCl (3.) 3.10 g KCl in 75.0 mL of 0.270 M CaCl2
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Calculate the molar concentration HCl when 250 mL of 0.10 M HCl are mixed with 150 mL of 0.10 M NaOH in a beaker. (5) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
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Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. K2SO:(aq) + FeCls(aq) – 1. 3. 6. () (aq) NR Fe K Reset 9, 4+ 2.
2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid 1.3 x 10-5 ) in a flask, and this was titrated with a 0.1895 M solution of (CH:CH-COOH) (Kа sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) 2.1.2 Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. 2.1.3 Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.