Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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A. A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.023 M HCl, and the equivalence point is reached after 36.5 mL of titrant are dispensed. Based on this data, what is the concentration (M) ofCa(OH)2?
B. A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.026 M HCl, and the equivalence point is reached after 35.9 mL of titrant are dispensed. Based on this data, what is the concentration (M) of the hydroxide ion?
4. A solution of 2.5 x 104M NazS203 was used for the iodometric titration of an ozone-
containing sample. The titration volume was 10.00 mL NazS2O3.
a. Calculate the number of moles of Na2S2O3.
b. Calculate the number of moles of ozone in the sample.
A 25.0 mL sample of 0.723 M HCIO4 is titrated with a 0.135M Ba(OH)2 solution. The H3O+ concentration after the addition of 75.00 mL of Ba(OH)2 is? ______ M
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- The amount of oxygen, O2, dissolved in a water sample at 25 C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to MnO2. A solution of H2SO4 and KI is then added to convert the MnO2 to Mn2+, and the iodide ion is converted to I2. The I2 is then titrated with standardized Na2S2O3. (a) Balance the equation for the reaction of Mn2+ ions with O2 in basic solution. (b) Balance the equation for the reaction of MnO2 with I in acid solution. (c) Balance the equation for the reaction of S2O32 with I2. (d) Calculate the amount of O2 in 25.0 mL of water if the titration requires 2.45 mL of 0.0112 M Na2S2O3 solution.arrow_forwardIron (II) can be oxidized to iron (III) by dichromate ion, which is reduced to chromium (III) in acid solution. A 2.5000-g sample of iron ore is dissolved and the iron converted into iron(II). Exactly 19.17? ml. of 0.0100 M Na2Cr2O7 is required in the titration. What percentage of the ore sample was iron?arrow_forwardA solution contains 0.10 M iodide ion, I, and 0.10 M carbonate ion, CO32. (a) If solid Pb(NO3)2 is slowly added to the solution, which salt will precipitate first, Pbl2 or PbCO3? (b) What will be the concentration of the first ion that precipitates (CO32 or I) when the second, more soluble salt begins to precipitate?arrow_forward
- What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?arrow_forwardA solution contains 0.018 mole each of I, Br, and Cl. When the solution is mixed with 200. mL of 0.24 M AgNO3, what mass of AgCl(s) precipitates out, and what is [Ag+]? Assume no volume change. AgI:Ksp=1.51016AgBr:Ksp=5.01013AgCl:Ksp=1.61010arrow_forwardWhat is the Cl concentration just as Ag2CrO4 begins to precipitate when 0.90 M AgNO3 is slowly added to a solution containing 0.015 M Cl and 0.015 M CrO42?arrow_forward
- Consider the equation G = -nF. What are the four terms in this equation? Why does a minus sign appear in the equation? What does the superscript o indicate?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_forwardYou have a solution that contains AgNO3, Pb(NO3)2, and Cu(NO3)2. Devise a separation method that results in having Ag+ in one test tube, Pb2+ in another, and Cu2+ in a third test tube. Use solubility guidelines and Ksp and Kf values.arrow_forward
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