Write a charge balance for an aqueous solution of H2SO4 in water if the H2SO4 ionizes to HSO4- and SO42-
(1) Find the ionic strength of 0.020 MKBr plus 0.010 M Na2SO4 (2) Write the charge balance for a solution of HSO in water if the H2SO4 ionizes to HSO4 and SO42; 3) Explain why the solubility of an ionic compound increases as the ionic strength of the solution increases (at least up to -0.5 M). (30 points)
1- Calculating [H+] for Pure Water: In a certain acidic solution at 25 ∘C, [H+] is 100 times greater than [OH −]. What is the value for [OH −] for the solution? In a certain acidic solution at 25 , [] is 100 times greater than [ ]. What is the value for [ ] for the solution? 1.0×10−8 M 1.0×10−7 M 1.0×10−6 M 1.0×10−2 M 1.0×10−9 M 2. ± Acid-Base Relationships in Water: Water ionizes by the equation H2O(l)⇌H+(aq)+OH−(aq)The...
Calculate the concentrations of H2SO4, HSO4−, SO42− and H3O+ ions in a 0.12 M sulfuric acid solution at 25°C (Ka2for sulfuric acid is 1.3 × 10−2.) a). H2SO4 b). HSO4- c). SO42- d). H3O+
5. (2 points) Write the a) mass balance expression(s) and b) charge balance expression for barium sulfate, BaSO4, in 0.10 M HCl. The pertinent equilibria are: BaSO4(s) = Ba²+ + SO2- H3O+ + SO42- = HSO4 + H2O 2H,0 = H3O+ + OH
An aqueous solution of sulfuric acids, H2SO4, is reacted with with a 0.122 M solution of sodium hydroxide, NaOH. a. Write the balance equation. b. How many ml of sodium hydroxide are needed to neutralize 27.0 ml of 0.080 M of the sulfuric acid?
Select the charge balance equation for an aqueous solution of MnCl, that ionizes to Mn2+, Cl", Mncl. and MnOH! O [H+1+2 [Mn2+] + [MnCit] + [MnOH*] = [CI] + [OH"] O [H+] + [Mn2+1+[MnCit] + [MnOH"] = [CI"] + [OH"] O Mn²+1+[MnCit]+[MnOH] = 2 [CI"] 2 [Mn2+] + [MnCit] + [Mnoht] = [CH]+[OH"] O [H] + [Mn2++ [MnCit]+[MOH"] = 2 [C1") + (OH") O [Mn+1+ [MnCit] + [MnOH+] = 2 [C1"] + [OH"] O [Mn2+] + [MnC'] + [MnOH+] =...
Write the balanced neutralization reaction that occurs between H2SO4 and KOH in aqueous solution. Phases are optional. neutralization reaction: Suppose 0.750 L of 0.400 M H2SO4 is mixed with 0.700 L of 0.280 M KOH. What concentration of sulfuric acid remains after neutralization?
Write the balanced neutralization reaction that occurs between H2SO4 and KOH in aqueous solution. Phases are optional. neutralization reaction: Suppose 0.350 L of 0.490 M H2SO4 is mixed with 0.300 L of 0.200 M KOH . What concentration of sulfuric acid remains after neutralization?
For a 0.1 M aqueous solution of sodium acetate, Na+CH3CO2- , write two mass balance equations and a charge balance equation.
What are the concentrations of HSO4−, SO42−, and H+ in a 0.37 M KHSO4 solution? (Hint: H2SO4 is a strong acid; Ka for HSO4− = 1.3 × 10−2.)