Predicting precipitationComplete the table below by deciding whether a precipitate forms whenaqueous solutions A and B are mixed. If a precipitate will form, enter itsempirical formula in the last column.Does aempiricalprecipitate formsolution Asolution Bformula ofwhen A and Bprecipitateare mixed?sodium chlorideammonium nitrateyesnozinc chlorideammonium sulfideyesnonickel(II) sulfateiron(II) chlorideyesno

Given : We have to tell that precipitate will form or not.

Answered: Complete the table below by deciding…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter16: Solutions

Section: Chapter Questions

Problem 99E: The equation for a reaction by which a solution of sodium carbonate may be standardized is...

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For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble. Is Kc1,1 or 1 for a useful precipitation reaction?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
Solubility 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?
In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L [Mg2+]0 = 3.75 103 [F]0 = 6.25 102 reactstoformMgF2ymol/Mg2+ [Mg2+] = 3.75 103 y [F] = 6.25 102 2y
Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?
The following data apply to the unbalanced equation A(g)B(g) (a) On the basis of the data, balance the equation (simplest whole-number coefficients). (b) Has the system reached equilibrium? Explain.
Magnesite (magnesium carbonate, MgCO3) is a common magnesium mineral. From the solubility product constant, find the solubility of magnesium carbonate in grams per liter of water.
Suppose that an aqueous solution is in equilibrium with solid calcium sulfate and solid barium sulfate. What are the concentrations of calcium ion and barium ion in the solution?
calculate the new equilibrium composition of a system after an applied stress.
A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?

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