Calculate the pH of this solution
molar concentration of OH− ions in a 0.085 M solution of ethylamine (C2H5NH2; Kb=6.4×10−4).
[OH−]
[OH−] = |
7.1×10−3 | M |
Calculate the pH of this solution.
Express your answer to two decimal places.
Calculate the pH of this solution molar concentration of OH− ions in a 0.085 M solution...
Calculate the molar concentration of OH− ions in a 0.069 M solution of ethylamine (C2H5NH2 ; Kb=6.4×10−4
16)Calculate the molar concentration of OH− ions in a 0.074 M solution of ethylamine (C2H5NH2 ; Kb=6.4×10−4 ).
15. Calculate the molar concentration of OH− ions in a 0.074 M solution of ethylamine (C2H5NH2 ; Kb=6.4×10−4 ).
Calculate the molar concentration of OH-ions in a 0.084 M solution of ethylamine (C2H, NH2 ; Kb-6.4 × 10-4). Express your answer to two significant figures. OH] Previous Answers Request Answer
Part A Calculate the molar concentration of OH ions in a 0.555 M solution of hypobromite ion (BrO; Kb 4.0 x 10-) Express the molarity to two significant digits. V ΑΣφ ? [OH М What is the pH of this solution? Express the pH to two decimal places. VAD ΑΣφ ? pH=
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If a neutral solution of water, with pH = 7.00, is cooled to 10oC, the pH rises to 7.27. Which of the following three statements is correct for the cooled water: (i) [H+] > [OH-], (ii) [H+] = [OH-], or (iii) [H+] < [OH-]? 2) Calculate the pH of a 0.075 M solution of ethylamine (C2H5NH2; Kb = 6.4*10-4).
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