Concept explainers
Interpretation:
The chemical equations for the given series of reactions needs to be determined.
Concept introduction:
A chemical equation refers to the symbolic representation of a given
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General Chemistry: Principles and Modern Applications (11th Edition)
- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardCalculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.arrow_forwardThe photograph below shows what occurs when a solution of potassium chromate is treated with a few drops of concentrated hydrochloric acid. Some of the bright yellow chromate ion is converted to the orange dichromate ion. 2 CrO42(aq) + 2 H3O+(aq) CrO72(aq) + 3 H2O() (a) Explain this experimental observation in terms of Le Chateliers principle. (b) What would you observe if you treated the orange solution with sodium hydroxide? Explain your observation.arrow_forward
- 1) The following reaction was allowed to reach equilibrium at 25oC. Enclosed with the phase of each species is the equilibrium concentration. Calculate the equilibrium constant (Kc and Kp) for this reaction. 2 NOCl(g, 2.6 M) = 2 NO(g, 1.4 M) + Cl2(g, 0.34 M) 2) Calculate the pH of a 0.10 M hypochlorous acid solution. Ka = 3.5 x 10-8.arrow_forwardThe blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O Oarrow_forward-6 -5 -4 -3 -2 -1 +1 +2 +3 +4 +5 PbsO.(s) + H*(aq) + 2CI (aq) = Pb(s) + HSO. (aq) + Cl2(g)arrow_forward
- A 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL. After acidification, silver nitrate was added to a 25.00 mL aliquot where the resulting precipitate was filtered, washed and then redissolved in an ammoniacal solution of potassium tetracyanonickelate(II) according to the reaction: Ni(CN), + 2 AgBr) → 2 Ag(CN), + Ni? + 2 Br The liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate ion in a 10.00 mL aliquot was reduced to bromide with As* prior to the addition of silver nitrate. The same procedure was followed and the released nickel ion was titrated with 21.94 mL of the EDTA solution. Calculate the percentage of impurity in the sample. Br (79.904) a. 24.45% b.34.38% c. 41.17% d. 65.62%arrow_forwardWrite the balanced chemical reaction for this equilibrium expression: K= [H2O]P[O2] [H2O2]?arrow_forwardAn equilibrium reaction between chromate ions, CrO4 2- (yellow), and H+ ions is established to produce dichromate, Cr₂072- (orange). Note the colours. A student adds NaOH to a test tube containing an orange mixture of the above reagents. What is observed? 01. The solution turns from orange to yellow O 2.A precipitate forms 3. The solution tuimns from orange to colourless O4. The solution remains orangearrow_forward
- Co(H2O)62* (ag) +CF(ag) = CoCl42-(ag) + H2O (1) a) Balance this equation and write the expression for the equilibrium constant for this reaction. Write the expression for the equilibrium constant for this reaction. b) If the concentrations of all species are 2.50M at 25°C and the equilibrium constant of the reaction at 25°C is Keq = 2.85 102, how will the reaction shift? Show calculations and explanation. c) Explain the effect of adding silver nitrate to the solution. How does it shift the reaction? Provide the ionic equation.arrow_forwardWrite the K formula for the following reactions.arrow_forwardYou were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4. The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. In terms of Mg(OH)2 content, does the sample product conform to the USP requirement? Justify your answer through calculations.arrow_forward
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