What is the concentration of the unknown HCl solution in M?

What volume of base is required to reach the equivalence point in a titration of 20.00 mL of 0.11 M nitric acid with 0.25 M sodium hydroxide?

What's a definition of "Titration"

In a particular titration experiment a 30.0 mL sample of an unknown monoprotic acid required 25.0 mL of 0.200 M NaOH for the end point to be reached. What is the concentration of the acid?

If 27.9 mL of 0.200 M NaOH was required to reach the equivalence point in the titration of 100 mL of a weak acid, what was the initial concentration of the acid

A 0.478 g sample of an unknown strong base is dissolved in 50.0 mL of water and titrated with a 0.135 M HCL solution. The equivalence point is reached when a total of 29.0 mL of HCL is added. The base and acid conbine in a 1:1 ratio. (a) How many moles of base are neutralized when the equivalent point is reached? (b) What was the initial concentration (M) of this unknown base? (c) What is the molar mass of the unknown base?

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?

Please type this, do not write it on a paper.

A 21.6 mL sample of a 0.329 M aqueous acetic acid solution is titrated with a 0.379 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? pH =

A 0.658 g sample of a diprotic acid is dissolved in water and titrated with 0.130 M NAOH. What is the molar mass of the acid if 38.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. 10 11 12 13 molar mass: g/mol 18 19 20 21 22 23 24