In a titration, the equivalence point is achieved when the concentration of the base is equal to the concentration of the original acid. the pH changes. a solution is partially neturalized. the moles of acid and base are equal.

For the titration of 3.00 M hydrochloric acid with 2.00 M sodium hydroxide, what volume of sodium hydroxide would be required to react with 1.00 L of hydrochloric acid to reach the endpoint?

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

A student conducting this experiment measures out 0.913 g of an unknown monoprotic weak acid and dissolves it in 110 mL of water. After adding an indicator, the student titrates the weak acid with 15.55 mL of 0.380 M NaOH to reach the equivalence point. What is the molar mass of the unknown acid?

A chemistry graduate student is given 125.mL of a 0.40M ammonia NH3 solution. Ammonia is a weak base with Kb = 1.8x10−5. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.03? You may assume that the volume of the solution doesn't change when then NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

The table has data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCl(aq), using a 0.299 mol/L sodium hydroxide standard solution.   Titration of 10.0 mL HCl(aq) with 0.299 mol/L NaOH(aq) Trial #1 #2 #3 #4 final burette reading (mL) 17.9 35.0 22.9 40.1 initial burette reading (mL) 0.3 17.9 5.9 22.9 volume of NaOH(aq) added (mL)         colour at endpoint blue green green green a)  Select the most consistent trials and calculate the average volume of titrantadded.b)  Calculate the concentration of the hydrochloric acid solution.

A sample of 25.0 mL of buffer solution contains 0.100 M fluoride ions and 0.126 M hydrofluoric acid. If 4.93 mL of 0.0100 M HCI are added to the sample, what is the resulting concentration of fluoride ions?

What is an indicator? What is a buffer?

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:

The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl.  How would you classify the species being titrated in this titration? diprotic weak base monoprotic weak base triprotic weak acid triprotic weak base diprotic weak acid monoprotic weak acid