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Consider the reaction
(b) Will more AgCl precipitate if H+ ions are added?
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Chemistry: Principles and Reactions
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- Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.arrow_forwardCalculate the molarity of AgNO3 in a solution prepared by dissolving 1.44 g AgNO3 in enough water to form 1.00 L solution.arrow_forwardWhen 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?arrow_forward
- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardCopper(I) ions in aqueous solution react with NH3(aq) according to Cu+(aq)+2NH3(aq)⟶Cu(NH3)+2(aq) ?f=6.3×10^10 Calculate the solubility (in g·L−1) of CuBr(s) (?sp=6.3×10^−9) in 0.47 M NH3(aq). solubility of CuBr(s): g/Larrow_forwardA reaction is initiated by preparing an aqueous solution with 0.421 M silver ion, Ag+ (aq), and 0.778 M ammonia, NH3 (aq). The following reaction proceeds until equilibrium is achieved. Ag+ (aq) + 2 NH3 (aq) = [Ag(NH3)2]+(aq) At equilibrium, it is determined that the solution contains 0.292 M [Ag(NH3)2]+ (aq). The value of K is Write your answer to 3 sig figs (ie. 1.23E1)arrow_forward
- A chemist wishes to precipitate yttrium cations out of a 1.00 L solution. if the concentration of (in solution is 0.428 M and the K of yttrium iodate is 1.12 x 10, what mass of potassium lodate (00 must be added so that precipitation may begin? The molar mass of potassium lodate is 21A.00 g/mol. (27) (A) (B) (C) (D) 91.6g 64.0 ug (6.4 x 10* g) 411 mg 56.0 ng 137 mg (5.6 x 10* g) (E)arrow_forwardLimestone consists mainly of the mineral calcite, CaCO 3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO 2: CaCO 3(s) + 2 HCl → CaCl 2 + CO 2(g) + H 2O The excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.arrow_forwardAn analytical chemist has a solution containing chloride ion, Cl¯. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AGNO3. As a way to indicate the endpoint of the titration, she added 1.13 g of potassium chromate, K2CrO4. As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.8 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations. Ksp for Ag, CrO4 is 1.1 x 10-12, K, for AgCl is 1.8 x 10-10 moles of Cl¯ in the original solution moles of Cl¯ in the final solutionarrow_forward
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