For each, write the chemical equation for its dissociation in water: a. Co(NO3)2 b. Cu(NO3)2 + С. Ni(NO3)2 Hint: All three are ionic compounds that follow the principle described in this video: https://www.youtube.com/watch?v=ZOGEKX7OJHS What must account for the different colors?

For each, write the chemical equation for its dissociation in water: a. Co(NO3)2 b. Cu(NO3)2 + С. Ni(NO3)2 Hint: All three are ionic compounds that follow the principle described in this video: https://www.youtube.com/watch?v=ZOGEKX7OJHS What must account for the different colors?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter7: Reactions In Aqueous Solutions

Section: Chapter Questions

Problem 8QAP: ow do chemists know that the ions behave independently of one another when an ionic solid is...

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Which ion(s) are responsible for making water “hard”? a. Na+, Ca2+, and Mg2+ b. Ca2+ c. Mg2+ d. Ca2+ and Mg2+ e. Na+ f. None of these ions are responsible for making water "hard".
1. What is the difference between chemical species, an ion, and an element?2. Provide examples of all possible reactions that can occur in soils.3. By what mechanisms are ions held by soils?4. How is soil chemistry knowledge useful to agriculturalists and environmentalists?
Metal cations in solution are complexed to H2O molecules and exist as hydrated ions. For example, Ni2+ complexes to form the hydrated ion Ni(H2O)62+. Metal cations are also able to complex to other ligands, such as NH3. Part 1 An aqueous solution is prepared in which 0.00166 mol Ni(NO3)2 and 0.353 mol NH3 are dissolved in a total volume of 1.00 L.Classify the species present in the resulting solution according to their relative amounts. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Part 2 Write the expression for the dissociation constant needed to determine the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed in Part 1. Kd = ___________ Part 3 Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed. ______ M Please answer all three parts.
Metal cations in solution are complexed to H2O molecules and exist as hydrated ions. For example, Ni2+ complexes to form the hydrated ion Ni(H2O)62+. Metal cations are also able to complex to other ligands, such as NH3. An aqueous solution is prepared in which 0.00139 mol Ni(NO3)2 and 0.353 mol NH3 are dissolved in a total volume of 1.00 L.Classify the species present in the resulting solution according to their relative amounts. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Ions in Solution (2 items) (Drag and drop into the appropriate area below) Do not place spaces in your answer. Write the expression for the dissociation constant needed to determine the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed in Part 1. Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed.
4 g of magnesium nitrate is dissolved in 1.20 L of water. 25 mL of this solution is taken and diluted to 175 mL with water. What is the final concentration of the nitrate ion?
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Metal cations in solution are composed to H2O molecules and exist as hydrated ions. For example, Ni^2+ complexes to form the hydrated ion Ni(H2O)6^2+. Metal cations are also able to complex to other ligands, such as NH3. Part 1: An aqueous solution in which 0.00166 mol Ni(NO3)2 and 0.353 mol NH3 are dissolved in a total volume of 1.00 L. Classify the species present in the resulting solution according to their relative amounts. Kf for Ni(NH3)^2+ is equal to 5.5*10^8. The part that I need help on is part 3: calculate the concentration of Ni(H2O)6^2+ ions at equilibrium in the solution formed.
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