Solved

What Is the Hydronium Ion Concentration of a 0

Question 36

Multiple Choice

What is the hydronium ion concentration of a 0.500 mol L-1 acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below: What is the hydronium ion concentration of a 0.500 mol L<sup>-1</sup> acetic acid solution with K<sub>a</sub> = 1.8 × 10<sup>-5</sup>? The equation for the dissociation of acetic acid is below: A) 3.0 × 10<sup>-2</sup> mol L<sup>-1</sup> B) 4.2 × 10<sup>-2</sup> mol L<sup>-1</sup> C) 3.0 × 10<sup>-3</sup> mol L<sup>-1</sup> D) 4.2 × 10<sup>-3</sup> mol L<sup>-1</sup>


A) 3.0 × 10-2 mol L-1
B) 4.2 × 10-2 mol L-1
C) 3.0 × 10-3 mol L-1
D) 4.2 × 10-3 mol L-1

Correct Answer:

verifed

Verified

Unlock this answer now
Get Access to more Verified Answers free of charge

Related Questions

Q33: Calculate the pH of a 1.60 mol

Q33: Calculate the hydroxide ion concentration in an

Q35: A 7.0 × 10<sup>-3</sup> mol L<sup>-1</sup> aqueous

Q37: Calculate the pH for an aqueous solution

Q39: Which one of the following will form

Q44: Determine the [OH⁻] concentration in a 0.169

Q84: Calculate the pOH of an aqueous solution

Q96: Determine the [OH<sup>-</sup>] concentration of a 0.116

Q120: Describe a molecule that can be a

Q121: Which of the following equilibria represents the