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_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_forwardCalculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.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_forwardA 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_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
- 4. Which cation or cations may be present in a pale blue solution that turns deep blue and forms a white precipitate upon addition of 6 M NH,(aq)?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_forwardCo(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_forward
- Write the balanced chemical reaction for this equilibrium expression: K= [H2O]P[O2] [H2O2]?arrow_forwardWrite the K formula for the following reactions.arrow_forwardThe solubility of Cl, in 100 g of water at STP is 310 cm³. Assume that this quantity of Cl2 is dissolved and equili- brated as follows: Cl2(aq) + H20 = cl (aq) + HCIO(aq) + H*(aq) (a) If the equilibrium constant for this reaction is 4.7 x 10-, calculate the equilibrium concentration of HCIO formed. (b) What is the pH of the final solution?arrow_forward
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