A 46.91 mL solution of weak acid is titrated with 0.429 M NaOH. It requires 34.58 mL of the NaOH titrant to reach the equivalence point. Based on the titration curve, it is determined that K = 5.6 x 10-7 for the weak acid. Please note that you can use the above information, and a given volume of NaOH titrant added, to calculate the pH at any point along a titration curve. In this assignment, several questions will walk you through intermediate steps, such as this first question asking for the molarity of weak acid. For quiz assignments, expect questions that ask about the pH of the solution only. Based on the above information, what was the initial concentration of the weak acid before any NaOH was added? Write your answer to 3 significant figures. Answer: Based on this same prompt, what was the initial pH before any NaOH was added? Write your answer to 2 decimal places (ie. 1.23 or 12.34). Answer: Based on this same prompt, how many moles of the conjugate base have formed after 18.673 mL of the NaOH titrant was added? Write your answer to 3 significant figures. Note that in general I will not ask this question. This is an intermediate step along the way to finding the pH. Please focus on being able to calculate the pH at each point during an acid-base titration. Answer: Based on this same prompt, how many moles of the weak acid remain in solution after 18.673 mL of the NaOH titrant was added? Write your answer to 3 significant figures. Note that in general I will not ask this question. This is an intermediate step along the way to finding the pH. Please focus on being able to calculate the pH at each point during an acid-base titration. Answer: