Concept explainers
(a)
Interpretation:
Out of
Concept Introduction:
The solubility product for an equilibrium reaction is defined as the product of ion concentration raised to power their
The precipitation takes place due to the different solubilities of the two ionic compounds. The compound which is more soluble will remains in the solution whereas less soluble compound precipitates first.
(b)
Interpretation:
The concentration of first anion species when second anion species starts to precipitate has to be calculated.
Concept Introduction:
The solubility product for an equilibrium reaction is defined as the product of ion concentration raised to power their stoichiometric coefficient. The symbol for solubility product is
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OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
- Solubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume that you have 1.0 L of solution in each case. a Are there any beakers where you would observe solid still present? How do you know? b Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations. c For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2, compare? (You dont need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer. d Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need? e Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information? f How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?arrow_forwardSuppose that an aqueous solution is in equilibrium with solid calcium sulfate and solid barium sulfate. What are the concentrations of calcium ion and barium ion in the solution?arrow_forwardConsider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of barium nitrate is added. Assuming no change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.arrow_forward
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- Write the precipitation reaction for ammonium bromide in aqueous solution: Is ammonium bromide considered soluble or not soluble ?arrow_forwardIn this assignment, you will determine the mass % of an unknown sample of baking soda (NaHCO3) by titrating it with an HCl solution of known concentration. The laboratory will open with a beaker on the stir plate with 1.5000 g of impure solid NaHCO3 and with sufficient water added to make the total volume 25.00 mL. The buret will be filled with 0.3015 M HCl. Pouring HCI until pH is 2. The volume in the buret went from 0 mL to 43 mL Question 1: Calculate the moles of HCl transferred during the titration. (number and unit) (Keep four significant digits in all of the calculations.) Question 2: How many moles of NaHCO3 are present in the sample? Question 3: What mass of NaHCO3 is present in the sample? Question 4: What percent of the original sample mass was NaHCO3?arrow_forwardThe molar solubility of lead chromate in a 0.214 M potassium chromate solution is M.arrow_forward
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