Visited A solution contains 7.44x10-3 M lead nitrate and 1.43x10-2 M calcium acetate. Solid sodium phosphate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of phosphate ion when this precipitation first begins? [PO4³] = Submit Answer M Retry Entire Group 8 more group attempts remaining

Visited A solution contains 7.44x10-3 M lead nitrate and 1.43x10-2 M calcium acetate. Solid sodium phosphate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of phosphate ion when this precipitation first begins? [PO4³] = Submit Answer M Retry Entire Group 8 more group attempts remaining

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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1. A 12.5 mL volume of 0.500 M H2SO4 neutralizes 50.0 mL of NaOH. A. What is the acid (formula and name)? B. What is the base (formula and name)? C. Write a balanced chemical equation for the reaction. D. Write the complete ionic equation for the reaction. E. Write the net ionic equation for the reaction. F. What is the concentration of the NaOH solution? (This is a titration).
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5) Which combination will produce a precipitate? 1-3 A. Cu(NO3)2 (aq) and KC2H3O2 (aq) B. AgC2H3O2 (aq) and HC2H3O2 (aq) C. NaOH (aq) and Sr(NO3)2 (aq) D. Pb(NO3)2 (aq) and HCl (aq) recipitation
Rb
12. In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 L if acid in a flask. You quickly add 20.00 mL of 0.0502 M NaOH but overshoot the endpoint, turning the solution a deep pink color. Instead of starting over you add an additional 30.00 mL of the acid, turning the solution colorless. It then takes 3.22 mL of the NaOH to reach the endpoint. a. Write the Molecular, Total Ionic, and Net Ionic Equations for this reaction. b. What is the concentration of the HNO3 solution? c. How many moles of NaOH were in excess after the first addition?
The four solutions were made and then mixed in the following order. 1. Starting with 0.100M Bacl2 100.0 mL 2. Adding 0.100M AgNo3 50.0 mL 3. Adding 0.100M H2SO4 50.0 mL 4. Added 0.100M NH3 250.0 mL Write a response formula for the response that takes place after each step, assume that all the responses are complete and calculate the concentration of Ba2+, Cl-, NH3 and NH4+ in the final solution.