The antacid "TUMS" was titrated using 0.3 M HCl. The buret reading was initially 2.67 mL. After reaching the endpoint, the final volume reading was 21.04 mL. What volume of HCl was used in this titration? Include a unit in your answer.

A 15.5 mL sample of 0.800 M NaOH was titrated with an acid. It required 25.0 mL of the acid to reach the equivalence point. The molarity of the acid is

QUESTION 5 Consider the titration of 17.7 mL of 0.211 M HNO3 with 0.130 M NaOH solution. What volume (in L) of NaOH is required to reach the equivalence point in the titration? Give your answer in numerical form (NOT exponential notation) using the correct number of significant figures. Lavide jon.

Please help me find the initial concentration of acid (M). This is a titration. Volume of acid (mL): 10.0 Volume of NaOH at equivalence point (mL): 30.1 Milimoles of NaOH to neutralize the acid: 50.0 Milimoles of acid: 50.0 Also could you help me find the average initial concentration?

A sample of oxalic acid (a diprotic acid of the formula H2C2O4) is dissolved in enough water to make 1.00 L of solution. A 100.0 mL sample of this solution is titrated with a solution of sodium hydroxide (NaOH) of concentration 0.750 M and requires 20.0 mL of sodium hydroxide to reach the end point. Calculate the mass of the original oxalic acid sample.H2C2O4 + 2NaOH → Na2(C2O4)+ 2H2OSelect one:A. 1.35 g B. 6.75 g C. 13.5 g D. 0.675 g

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4. How many mL of 0.100 M NaOH (aq) would be needed to completely neutralize 50.0 mL of 0.300 M HCI (aq)?

A 50.0 mL sample of aqueous sodium hydroxide is titrated with 0.425 M sulfuric acid, and 57 mL are required to reach the equivalence point. Write the balanced chemical equation for this reaction. Answer: A 50.0 mL sample of aqueous sodium hydroxide is titrated with 0.425 M sulfuric acid, and 57 mL are required to reach the equivalence point. What is the molarity of the initial sodium hydroxide solution? Hint: You will need the balanced chemical equation you provided as your answer to the previous question. Report your answer to the correct number of significant figures and with the correct units. Answer:

Answer both questions regarding Acids and Bases. After adding 50 mL of NaOH solution, the sample in the flask still had not turned pink. What error did the student make? and then, compare your percentage of HCI to the manufacturer’s percentage for the toilet bowl cleaner. We’re your results close? What might account for any differences? (Use the second photo for reference)

24.16 mL of 0.2704 M sodium hydroxide is titrated with 29.00 mL of phosphoric acid.  Calculate the molarity of phosphoric acid.