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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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2. Several highly toxic substances were found in the white river, including heavy metal waste from plating solutions and sludge. These heavy metal ions (Cu 2+, Cr3+, and Ni2+) can be removed by reacting with sodium hydroxide to form insoluble metal hydroxides. Write balanced chemical equations for the following precipitation (double displacement) reaction:
A) CuSO4 + NaOH —>
B) Cr 2(SO 4)3 + NaOH —>
C)NiSO 4 + NaOH —>
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- Consider the following chemical reaction. 3 Zn(C₂H₃O₂)₂(aq) + 2 Na₃PO₄(aq) → 6 NaC₂H₃O₂(aq) + Zn₃(PO₄)₂(s) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C₂H₃O₂)₂ in 105 mL H₂O. What is the concentration of this zinc acetate solution?arrow_forwardExp # 2: suppose you have a {Zn2+(aq), Fe3+(aq)} solution, and you’re asked to separate the two ions, how do you seperate the ions and form a precipitate?arrow_forwardAntacid tablets contain a variety of bases such as NaHCO3, MgCO3, CaCO3, and Mg(OH)2. Only NaHCO3 has appreciable solubility in water. A net ionic equation will not include spectator ions, but must include states of matter. Write the net ionic equation for Mg(OH)2 + HCl Choose the best answer to explain how insoluble substances can act as effective antacids.Choose one: Even as a solid, the antacid will react with H+ to neutralize the acid A small portion of the solid dissolves and neutralizes the acid The volume of the solid decreases the acid concentration, causing the pH to rise.arrow_forward
- Calculate the number of milliliters of 0.779 M KOH required to precipitate all of the Pb²* ions in 122 mL of 0.541 M Pb(NO3)2 solution as Pb(OH)2. The equation for the reaction is: Pb(NO3)2(aq) + 2KOH(aq) –→Pb(OH)2(s) + 2KNO3(aq) mL KOHarrow_forwardWrite a net ionic equation for the following precipitation reaction: KOH and Zn(NO3)2arrow_forwardWhat volume in mL of 0.38 M HBr solution is required to titrate 125mL of a 0.18 M Ca(OH)2 solution? Ca(OH)2(aq) + 2HBr(aq) -> CaBr2(aq) + H2O(I)arrow_forward
- A 65.0 mL sample of a 0.110 M potassium sulfate solution is mixed with 36.5 mL of a 0.114 M lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g . Determine the limiting reactant, the theoretical yield, and the percent yield.arrow_forwardAn unknown hydroxide of the formula X(OH)2 is only slightly soluble in water. A scientist is curious as to what hydroxide this is. So, she takes this hydroxide and dissolves enough of it in pure water to make a saturated solution. She then takes 25.00 mL of the saturated solution and titrates it with 0.000100 M HCl. She notes that it takes 2.58 mL of HCl to fully neutralize the saturated solution. 1. Determine the Ksp of the hydroxide. (concentration of X(OH)2 is 1.032 x 10-5 M, pH = 9.31, molar solubility should be 1.032 x 10-5 M)arrow_forwardA sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s) How many moles of Ag+ (aq) ions are used to reach the end point? How many moles of Cℓ- (aq) have reacted in the titration? How many grams of chloride are present in the sample? What is the mass percent of chloride in the sample?arrow_forward
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