k2=[H][SO4]/[HSO4] .012=(.01+x)(x)/(.01-x) Solve for x,

Calculate the pH of the following aqueous solution:1.00 mol/L sulfuric acid, H2SO4(aq) H2SO4 ==> H^+ + HSO4^- 100% HSO4^- ==>
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2. asked by Sarah
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Calculate the pH of the following aqueous solutions:1.00 mol/L sulfuric acid H+ = 1.00 M for the first ionization THe second one
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2. asked by Ross
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DrBob has given you the equation to use:k2 = [H^+][SO4^-]/[HSO4^-] and the values to substitute [H^+] = 0.01 + x [SO4^-2] = x
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2. asked by lyne
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Calculate the molar solubility of BaSO4 in a solution in which [H3O+] is 2.5 M.I can almost solve this on my own. If you know
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2. asked by Jay
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1- Calculate the equilibrium concentration for H+, HSO4- and SO4^2- , given a .150M H2SO4 solution. the Ka for HSO4- is
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2. asked by JOJO
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Complete these Brønsted-Lowry reactions:HSO4- + H+ <--> HSO4- +OH- <-->
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2. asked by Melissa
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate
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2. asked by Admir
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Identify the two conjugate acid-base pairs in each of the following:A) H2PO4^-(aq) + HSO4^-(aq) = H3PO4(aq) + SO4^2-(aq) B)
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2. asked by Robyn
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H2SO4(aq)+H2O(l)→H3O+(aq)+HSO4−(aq)solve
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2. asked by jessica
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k2=[H][SO4]/[HSO4].012=(.01+x)(x)/(.01-x) Solve for x, and calculate pH where H is .01+x When I am solving for x does it become
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2. asked by lyne
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