HClO4 + H2O = H3O+(aq) + ClO4-(aq)
HClO4 is strong acid and will dissociate completely.
H3O+ = HClO4 = 0.25 M
OH- = 10^-14 / H3O+
= 10^-14 / 0.25
= 4.00*10^-14 M
Calculate the concentrations of H3O+ and OH- ions in a 0.25 M HClO4 solution.
What are the concentrations of H3O+ and OH- ions (in M) in an aqueous solution with a pOH of 10.17? Is this solution acidic or basic? Explain your answer.
1. For the strong acid solution 0.0098 M HClO4, determine [H3O+] and [OH−]. Express your answers using two significant figures. Enter your answers numerically separated by a comma. For this solution determine pH. 2. For the strong acid solution 7.5×10−3 M HBr, determine [H3O+] and [OH−]. For this solution determine pH. 3. For the strong acid solution 3.77×10−4 M HI, determine [H3O+] and [OH−]. 4. For this solution determine pH. For the strong acid solution 0.0978 M HNO3, determine [H3O+]...
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+
Calculate the hydronium ion, H3O , and hydroxide ion, OH–, concentrations for a 0.0210 M NaOH solution.
NaOH (s) was added to 1.0L of HClO4 (aq) 0.49 M. a) Calculate [H3O+] in the solution after the addition on 0.11 mol of NaOH (s) b) Calculate [H3O+] in the solution after the addition of 0.84 mol of NaOH (s)
Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]= M Solution B:[H3O+]=8.91×10−9 M Solution B: [OH−]= M Solution C:[H3O+]=7.61×10−4 M Solution C: [OH−]= M Which of these solutions are basic at 25 °C? A:[OH−]=2.59×10−7 M B:[H3O+]=8.91×10−9 M
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Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 1.0×10−9 M . Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 2.3×10−2 M . Calculate [H3O+] in the following aqueous solution at 25 ∘C: [OH−]= 6.1×10−12 M . Classify the solutions as acidic or basic. [OH−]=1.0×10−9 M[OH−]=1.0×10−9 M [OH−]=2.3×10−2 M[OH−]=2.3×10−2 M [OH−]=6.1×10−12 M[OH−]=6.1×10−12 M
What is the pH of a 0.25 M solution of HCLO4 (perchloric acid)?