Suppose a 0.048M aqueous solution of sulfuric acid (H₂SO4) is prepared. Calculate the equilibrium molarity of SOof sulfuric acid in the ALEKS Data resource.Round your answer to 2 significant digits.M☐ x10×2-You'll find information on the properties pk, of weak acids at 25°NameFormulapKatpKa2pKa3acetic acidCHCOTH4.756benzoic acid4.204butanoic acidCHICOH4.834-chlorobutanoic acidC₂H CICO₂H4.52crotonic acidCHICOH4.69oxalic acidH₂C₂O1.253.81phosphoric acidH₂POA2.167.2112.32propionic acidCHCOM4.87sulfuric acidH₂SOAstrong acid1.99trimethylacetic acid5.03

Step 1: H2SO4, or sulfuric acid, is a diprotic acid. It's capable of giving out two protons. It is a…

Answered: Suppose a 0.048M aqueous solution of…

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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Either sulfuric acid or bismuth(III) nitrate pentahydrate can catalyze this reaction. What is an advantage to using sulfuric acid? What is an advantage of using the bismuth compound?
A student titrates a 35.00 mL sample of 0.0100 M sodium hypochlorite (NaClO), a salt containing the conjugate base of hypochlorous acid (HClO, Ka = 3.0 x 10-8), with 0.0125 M HCl. NaClO(aq)+ HCl(aq) → NaCl(aq)+ HClO(aq) Determine the pH after 12.00 mL of HCl has been added.
can be used as a standard solution for checking the concentration of a solution containing sulphuric acid, 8.7 cm' of sulphuric acid. Find the concentration of the sulphuric acid in both mol dm3 and g dm³. In a particular experiment 10,0 cm³ of a 0.50 mol dm³ solution of sodium ethanedioate was found to react with Q2. Sodium ethanedioate, Na;C¿O4, can be made into a solution of an exact and reliable concentration and so London ndon A.C.1.2
Chemistry
Calculate the concentration of HCO3 in an aqueous solution of 0.1120 M carbonic acid, H,CO3 (aq). [НСО3]%3D M.
NaOH 0.0963M
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Write a neutralization reaction for each acid and base pair. HClO4(aq)and Sr(OH)2(aq) Express your answer as a balanced chemical equation. Identify all of the phases in your answer.
If cobalt(II) sulfate is heated too strongly, the following reaction will occur CoSO4(s) à CoO(s) + SO3(g) If you are heating a sample of CoSO4·6H2O and this reaction occurs along withdehydration, what will happen to the experimental percent water? Explain your answer.
3. Sulphuric acid (H2S04 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1 = 1x 10° and Ka2 = 1.2 x 10¬2 The initial concentration of sulphuric acid is given as 0.040M. (i) Write the dissociation reactions. (ii) Calculate the concentration of [HSO, ] and [So? ]. (iii) Calculate the pH of the acid solution.
chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl (aq), as described by the chemical equation MnO2 (s) + 4 HCl (aq) -> MnCl2 (aq) + 2 H2O (l) + Cl2 (g) How much MnO2 (s) should be added to excess HCl (aq) to abtain 145 mL Cl2 (g) at 25 degrees celsius and 735 Torr? Mass of MnO2 = ? g
[References] Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas ( CH4) by the following process: 2NH3 (g) + 30,(g) + 2CH, (g) →→ 2HCN(g) + 6H,0(g) Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reaction vessel contains 5.75 g NH3, 12.0 g 02, and 5.00 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written? Mass = HCN

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