Concept explainers
(a)
Interpretation: The balanced molecular equation for the formation of
Concept introduction: The
(b)
Interpretation: The balanced molecular equation for the formation of
Concept introduction: The chemical reaction in which two salts solutions are mixed together and leads to the formation of solid residue is termed as precipitation reaction. The insoluble solid residue so formed is called precipitate. The chemical equation in which molecules of reactants and products are present is termed as molecular equation.
(c)
Interpretation: The balanced molecular equation for the formation of
Concept introduction: The chemical reaction in which two salts solutions are mixed together and leads to the formation of solid residue is termed as precipitation reaction. The insoluble solid residue so formed is called precipitate. The chemical equation in which molecules of reactants and products are present is termed as molecular equation.
(d)
Interpretation: The balanced molecular equation for the formation of
Concept introduction: The chemical reaction in which two salts solutions are mixed together and leads to the formation of solid residue is termed as precipitation reaction. The insoluble solid residue so formed is called precipitate. The chemical equation in which molecules of reactants and products are present is termed as molecular equation.
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Chemical Principles
- Use the solubility rules (Table 4.1) to decide which of the following compounds are expected to be soluble and which insoluble. a Mg(C2H3O2)2 b NiS c Cr(NO3)2 d Ca3(PO4)2arrow_forwardWhen the following solutions are mixed together, what precipitate (if any) will form? a. FeSO4(aq) + KCl(aq) b. Al(NO3)3(aq) + Ba(OH)2(aq) c. CaCl2(aq) + Na2SO4(aq) d. K2S(aq) + Ni(NO3)2(aq)arrow_forwardThree acid samples are prepared for titration by 0.01 M NaOH: 1 Sample 1 is prepared by dissolving 0.01 mol of HCl in 50 mL of water. 2 Sample 2 is prepared by dissolving 0.01 mol of HCl in 60 mL of water. 3 Sample 3 is prepared by dissolving 0.01 mol of HCl in 70 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). b When the titration is performed, which sample, if any, will require the largest volume of the 0.01 M NaOH for neutralization?arrow_forward
- The cations Ba2+ and Sr2+ can be precipitated as very insoluble sulfates. (a) If you add sodium sulfate to a solution containing these metal cations, each with a concentration of 0.10 M, which is precipitated first, BaSO4 or SrSO4? (b) What will be the concentration of the first ion that precipitates (Ba2+ or Sr2+) when the second, more soluble salt begins to precipitate?arrow_forwardSolubility 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_forwardWhen the following solutions are mixed together, what precipitate (if any) will form? a. Hg2(NO3)2(aq) + CuSO4(aq) b. Ni(NO3)2(aq) + CaCl2(aq) c. K2CO3(aq) + MgI2(aq) d. Na2CrO4(aq) + AlBr3(aq)arrow_forward
- A solution contains Ca2+ and Pb2+ ions, both at a concentration of 0.010 M. You wish to separate the two ions from each other as completely as possible by precipitating one but not the other using aqueous Na2SO4 as the precipitating agent. (a) Which will precipitate first as sodium sulfate is added, CaSO4 or PbSO4? (b) What will be the concentration of the first ion that precipitates (Ca2+ or Pb2+) when the second, more soluble salt begins to precipitate?arrow_forwardUse the solubility rules (Table 4.1) to decide which of the following compounds are expected to be soluble and which insoluble. a AgBr b Ca(NO3)2 c MgI2 d PbSO4arrow_forwardAccording to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?arrow_forward
- 1. Once a chemical equilibrium has been established, only the forward reaction occurs. only the reverse reaction occurs. the forward and reverse reactions occur at an equal rate. the forward and reverse reactions stop.arrow_forwardThere are many ionic compounds that dissolve in water to a very small extent. One example is lead(II) chloride. When it dissolves an equilibrium is established between the solid salt and its component ions. Suppose you stir some solid PbCl2 into water. Explain how you would prove that the compound dissolves but to a small extent? Is the dissolving process product-favored or reactant-favored? pbcl2(s)pb2+(aq)+2cl(aq)arrow_forwardDecide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction. (a) potassium nitrate and magnesium sulfate (b) silver nitrate and potassium carbonate (c) ammonium carbonate and cobalt(lll) chloride (d) sodium phosphate and barium hydroxide (e) barium nitrate and potassium hydroxidearrow_forward
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