For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.) manganese(II) hydroxide 2. iron(III) hydroxide Ksp 1. manganese(II) hydroxide = Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water. A. Ag₂SO4 B. AgCl C. Ksp = Cr(OH)3 D. Cas iron (III) hydroxide Note: Multiply out any number and put it first in the Ksp

For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.) manganese(II) hydroxide 2. iron(III) hydroxide Ksp 1. manganese(II) hydroxide = Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water. A. Ag₂SO4 B. AgCl C. Ksp = Cr(OH)3 D. Cas iron (III) hydroxide Note: Multiply out any number and put it first in the Ksp

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Pleasen help with this chemistry question.
1. The acid form of bromophenol blue (???) is yellow; the base form (??−) is blue. Approximately what wavelength of visible light do you think each of these forms will absorb? Briefly explain. 2. Solution ?3 is considered to be the acid form of the indicator. Solution ?3 is considered to be the basic form of the indicator. Consider Le Chatelier’s Principle and explain why this is so.
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3. What is the pH of a buffer produced by mixing 225 mL of 0.305 M HCOOH with 175 mL of 0.141 M KCOOH? Be sure to first find the new concentration of each compound in the mixed solution (M₁V₁ = M₂V₂ remember V₁ = total volume), then apply equilibrium.
4. Why is the pH at the equivalence point slightly different from that of the end point? Explain.
2. No need to explain too much
Given: 0.300M NaOH 35.0L of 0.450M CH3COOH solution. CH3COOH dissociate constant = 1.8*10^-5 write out the equilibrium equation formed at the equivalence point.
You are given a solution of 0.20M CoCl3, 0.15M SnCl2, 0.35M CuCl2, and 0.25M AgCl.Giventhe following table, calculatethe hydroxide concentration needed to precipitate each metal individually so they can be recovered. You do not want more than one metal to precipitate at one time or when you filter the precipitate you will get a mixture.(Optional; calculate the volume of a 0.25M NaOH solution needed to cause this precipitation) b.) Hydroxide needed to precipitate Sn(OH)2 c.) Hydroxide needed to precipitate Cu(OH)2 d.) Hydroxide needed to precipitate AgOH
7. For each of the following ionic compounds indicate whether the compound will be more soluble in pure water or an acidic solution. Explain. a. CdCO3(s) b. CUSCN(s)
Give the letters of the solutions below that represent buffers. (a) a solution of oxalic acid and potassium hydrogen oxalate; (b) a solution of formic acid and potassium formate; (c) a solution of potassium sulfate and potassium hydroxide; ( d) a solution of methylamine and methylammonium chloride.
How many milliliters of 1.27 M NaOH must be added to 275 mL of 0.11 M H₂PO4 to make a buffer solution with a pH of 6.407 Round your answer to 2 significant digits. Note: Reference the pK, of weak acids at 25 °C table for additional information,
How many moles of CH3NH.CI need to be added to 200.0 mL of a 0.500 M solution of CH&NH2 (Kb for CH.NH2 is 4.4 x 104) to make a buffer with a pH of 11.30? Type here to search