Elc. A JU student was asked to prepare a pH = 4.0 acid solution in which the molarity of His 1.0 x 10-4 M. The only acid that is available is sulfuric acid, H2SO4. Assume that H2SO4(1)will completely dissociate according to Eq. 1. H2SO4 (aq) S0 (aq)+2H* (aq)First, the student transferred 1.500 mL pure H2SO4 into a volumetric flask and made200.0 mL solution (solution 1). The density of pure H2SO4 is 1.84 g/mL. Then hetransferred exactly 10.00 mL solution 1 with a pipet into another volumetric flask andmade 250.0 mL solution (solution 2).Please calculate the molarities of both solutions for him. If he can solve this problemcorrectly, it will prove to his supervisor he has necessary skills.

GivenDensity of H2SO4= 1.84 g/mlVolume of H2SO4 taken= 1.500ml

Answered: Elc. A JU student was asked to prepare…

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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Professor Acetico Acido has assigned the analysis of unknown organic compound samples to Al Coholbased on their solubility behavior. The summary of the solubility profile are tabulated below along with thepossible structures of the samples. Identify each unknown sample by matching the respective solubility profilewith the given structures. Briefly explain the reason for your answer.
Swimming pool disinfectants produce hypochlorous acid upon dissolution. The weak acid ionizes as follows: HClO (aq) ⇄ H+ (aq) + ClO‒ (aq) Ka=3.0 x 10 ‒8 As strong oxidizing agents, both acid and its conjugate base kill bacteria. However, too high [HClO] is irritating to swimmers’ eyes and too high [ClO‒] will cause the ions to decompose in sunlight. The recommended pH to circumvent both problems is 7.8. Determine the ratio of the weak acid and its conjugate base at this pH.
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In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…
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You have found the following: CaSO4(s) <=> Ca+2(aq) + SO4-2(aq) K = (6.053x10^-5) What is the value of K for the following reaction? 2 CaSO4(s) <=> 2 Ca+2(aq) + 2 SO4-2(aq) Note: Your answer is assumed to be reduced to the highest power possible. Please provide neat and clean handwriting and clear image Give answer correctly
Predict the effect of adding H2O liquid to the equilibrium reaction
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Based on the first picture, answer the question on the second picture.

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