The hydronium-ion concentration of a 0.050 M solution of a weak acid is 5.1 time
ID: 1020634 • Letter: T
Question
The hydronium-ion concentration of a 0.050 M solution of a weak acid is 5.1 times 10^-3 M. The acid- dissociation constant is 1.37 times 10^4 at 25degree C. What is the pH of this solution? 5 28. 2.29 0.071 1.30 3.86 The density of ethane. C_2H_6 (30.1 g/mol.). at 28 degree C and 107 aim pressure is 1.34 g/L. 1.30 g/L. 0.767 g/L. 15.7g/L. 0.130g/L. A first -order chemical reaction is observed to have a rate constant of 23 min^-1. What is the corresponding half-life for the reaction? 32.9 s 1.8 min 2.6 s 1.8 s 33 min The volume of a sample of gas measured at 55.0degree C and 1.00 atm pressure is 8.00 L. What must the final temperature be in order for the gas to have a final volume of 2 00 L at 1.00 atm pressure? I039.0degree C -259.3 degree C 220.0degree C -191 0degree C 13.8degree CExplanation / Answer
34.
pH = -log (hydronium ion concentration)
pH = -log [H3O+ ]
pH = -log(5.1x10-3 )
pH = -(-2.29)
pH = 2.29
So, the correct option is B.
As per Chegg rule, it is allowed to answer only one question at a time.
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