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- When 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)When 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)Decide 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 hydroxide
- Three 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?Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed. (a) copper(II) sulfate and sodium chloride (b) manganese(II) nitrate and ammonium hydroxide (c) silver nitrate and hydrochloric acid (d) nickel(II) sulfate and potassium hydroxide (e) ammonium carbonate and sodium nitrateCalcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
- Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na2SO4 is added. Which cations could be present in the unknown soluble ionic compound?There 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)Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?
- Working with Concentration (Molarity Concepts) Note: You should be able to answer all of the following questions without using a calculator. Part 1: a Both NaCl and MgCl2 are soluble ionic compounds. Write the balanced chemical equations for these two substances dissolving in water. b Consider the pictures below. These pictures represent 1.0-L solutions of 1.0 M NaCl(aq) and 1.0 M MgCl2(aq). The representations of the ions in solution are the correct relative amounts. Water molecules have been omitted for clarity. Correctly label each of the beakers, provide a key to help identify the ions, and give a brief explanation of how you made your assignments. Keeping in mind that the pictures represent the relative amounts of ions in the solution and that the numerical information about these solutions is presented above, answer the following questions c through f. c How many moles of NaCl and MgCl2 are in each beaker? d How many moles of chloride ions are in each beaker? How did you arrive at this answer? e What is the concentration of chloride ions in each beaker? Without using mathematical equations, briefly explain how you obtained your answer. f Explain how it is that the concentrations of chloride ions in these beakers are different even though the concentrations of each substance (compound) are the same. Part 2: Say you were to dump out half of the MgCl2 solution from the beaker above. a What would be the concentration of the MgCl2(aq) and of the chloride ions in the remaining solution? b How many moles of the MgCl2 and of the chloride ions would remain in the beaker? c Explain why the concentration of MgCl2(aq) would not change, whereas the number of moles of MgCl2 would change when solution was removed from the beaker. As part of your answer, you are encouraged to use pictures. Part 3: Consider the beaker containing 1.0 L of the 1.0 M NaCl(aq) solution. You now add 1.0 L of water to this beaker. a What is the concentration of this NaCl(aq) solution? b How many moles of NaCl are present in the 2.0 L of NaCl(aq) solution? c Explain why the concentration of NaCl(aq) does change with the addition of water, whereas the number of moles does not change. Here again, you are encouraged to use pictures to help answer the question.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?Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.