A student is given a 0.1 M solution of an acid and is asked to determine whether it is a solution of a weak acid or a strong acid. The student measures the pH and determines it to be 2.3. Which of the following statements correctly identifies the strength of the acid and explain It is a strong acid, because the pH is greater than 1. B It is a weak acid, because the pH of a 0.1 M solution of a strong acid is 1. It is a weak acid, because the pH is less than 7. D) There is not enough information given to determine whether the acid is strong or weak.

Each of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are monoprotic, meaning that each acid molecule gives up one H+. The pH of each solution is as indicated.  Flask A: pH=1.1  Flask B: pH=2.4  Flask C pH= 2.9 Flask D: pH=5.1  How much strong base is required to neutralize the initial amount of acid? A. All four solutions will require the same amount of base because they all contain acid of the same concentration B. The solution of pH=1.1 will require the most base since it is the strongest acid and has the highest concentration of H+ C. Neither (A) nor (B) is correct.

The pH of an aqueous solution at 25°C was found to be 4.90. The pOH of this solution is . The hydronium ion concentration is M. The hydroxide ion concentration is M.

A chemist dissolves 698. mg of pure nitric acid in enough water to make up 350. mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.