Enter the chemical formulas of the soluble compounds MISSED THIS? Watch IWE7.6; Read Section 7.5. You can click onthe Review link to access the section in youreText.Pair each cation on the left with an anion on the right that will form asoluble compound and enter a formula for the soluble compound. Useeach anion only once.Na+NO3Sr2+So,2-Co2+ s2-Pb2+CO,2

Solubility of a salt depends upon the ion present in the salt. Given cations are Na+, Sr2+,…

SSED THIS? Watch IWE 7.6; Read Section 7.5. You can click on e Review link to access the section in your e Text. ir each cation on the left with an anion on the right that will form a uble compound and enter a formula for the soluble compound. Use ch anion only once. Na+ NO3 SO,2- Co2+ s2- Sr+ Pb?+ CO32-

SSED THIS? Watch IWE 7.6; Read Section 7.5. You can click on e Review link to access the section in your e Text. ir each cation on the left with an anion on the right that will form a uble compound and enter a formula for the soluble compound. Use ch anion only once. Na+ NO3 SO,2- Co2+ s2- Sr+ Pb?+ CO32-

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter15: Solutions

Section: Chapter Questions

Problem 62A

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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
n Chapter 14. you learned that the bonding forces in ionic solids such as NaCl are very strong, yet many ionic solids dissolve readily in water. Explain.
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It's a four part question a b and c are answered, I'm having trouble with d. I have no idea if a-c are correct. Consider a 1-L bottle of carbonated drink. The liquid is mostly water, and it can be assumed that its density is 1.00 g/mL. (a) Calculate the maximum moles of CO2 that can be dissolved in it. Use data that can only be found in the textbook. 1000 g / 44 g/mol = 2.27 g/mol (b) Calculate the % m/v of CO2 in this carbonated drink. 1 x 100 g = 100 g (c) What is the concentration of CO2 in ppm? 10^3 mg / 10^-3 L --> 10^6 mg/L = 10^6 ppm (d) If some of the 1-L carbonated drink is consumed, leaving 700 mL drink in the bottle. What is the concentration of CO2 in ppm in the drink that’s left in the bottle?
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1. What weight of KCI and H₂0 are needed to make 250 g. of 5 % solution? 2. Suppose that 2.5 ml of 20% AgNO3 solution (density is 1.19 g/ml) was used to precipitate the chloride in a sample of sea water. What weight AgNO3 was in the solution used? 3. A 30% solution of ethanol in H₂O at 20°C has a density of 0.95 g/ml. What weight ethanol is contained in 750 ml. of solution?
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(Eqn. 3) 1 IO3− + 8 I− + 6 H+ → 3 I3− + 3 H2O (Eqn. 4) 2S2O32− + I3− → 3I− + S4O62− Multiply Equation 4 by the molar ratio 3/1 and add to Equation 3 to obtain the overall balanced net ionic equation for the standardization of Na2S2O3. 1. What is the molar ratio of S2O32− to IO3− in the overall net ionic equation?
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Milk of magnesia, an over-the-counter laxative, is a mixture of magnesium hydroxide [Mg(OH)2] and water. Because Mg(OH)2 is insoluble inwater (see Table 4.3), milk of magnesia is a suspension rather than a solution. The undissolved solid is responsible for the milky appearance ofthe product. When acid such as HCl is added to milk of magnesia, the suspended Mg(OH)2 dissolves, and the result is a clear, colorless solution.Write and balance the molecular equation, and then give the ionic and net ionic equations for this reaction.
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