Additional aspects of aqueous solution: 4. In a 50.0mL titration of a strong acid (HCl) with...

Additional aspects of aqueous solution:

4. In a 50.0mL titration of a strong acid (HCl) with a strong base (NaOH) calculate the pH when the following volumes of a 0.100M NaOH solution are added:

a.45.0mL

b.51.0mL

Solutions

Expert Solution

queen_honey_blossom answered 4 weeks ago

Next > < Previous

Related Solutions

consider the titration of a strong acid, HCL, with a strong base NaOH. The 35 ml...

consider the titration of a strong acid, HCL, with a strong base NaOH. The 35 ml of .1 M HCL is in the flask. What is the pH of the solution after 40 ml of .100 M NaOH has been added to to it?

Consider the titration of a weak base (B- ) with a strong acid (HCl). Draw (this...

Consider the titration of a weak base (B- ) with a strong acid (HCl). Draw (this can be hand drawn) a pH (not pOH) vs mL HCl graph (it will not look the same as the one in question #13; if you start with a weak base, will the pH be low or high? As H+ is added, will the pH increase or decrease?). Label the titration curve with letters A-E, and describe the relative quantities of the dissociated base...

20. An aqueous solution of nitric acid is standardized by titration with a 0.162 M solution...

20. An aqueous solution of nitric acid is standardized by titration with a 0.162 M solution of potassium hydroxide. If 27.1 mL of base are required to neutralize 20.7 mL of the acid, what is the molarity of the nitric acid solution? M nitric acid

titration of 50.0mL 0.50M NH3 with 0.50 M HCL. Kb(NH3)=1.8x10^-5 Plot the pH of the solution...

titration of 50.0mL 0.50M NH3 with 0.50 M HCL. Kb(NH3)=1.8x10^-5 Plot the pH of the solution after the addition of the following volumes of HCL using ICE tables. 0.00mL, 10.00mL, 20.0mL, 25.0mL, 30.0mL, 40.0mL, 50.0mL,, 60.0mL

Consider the titration of 0.100 M HCl, a strong acid, with 0.100 M NH3, a weak...

Consider the titration of 0.100 M HCl, a strong acid, with 0.100 M NH3, a weak base: HCL(aq)+NH3(aq)---NH4+(aq)+H2O(l) Calculate the pH at the following points in the titration when 25.0 mL of 0.0100 M NH3 is titrated with 0.100 M HCL. A. 0.0 mL of HCl added B. 10.0 mL of HCl added C. At equivalence point D. 35.0 mL of HCL added

A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of...

A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of 1.02 g/mL. The molality of hydrochloric acid in the solution is ____ m. B) An aqueous solution of iron(III) sulfate has a concentration of 0.192 molal. The percent by mass of iron(III) sulfate in the solution is ____ %.

If you add strong acid (such as HCl) to the Tris solution above(25mM solution in 200mL)...

If you add strong acid (such as HCl) to the Tris solution above(25mM solution in 200mL) you can lower the pH. Using the Henderson-Hasselbalch equation (H-H), calculate how much strong acid in mM is need to lower the pH from 10.4 to 8.0. Remember pKa is 8.2. You might start by determining the amount of acid and base you have at each pH using the H-H equation. Then compare the differences in this ratio between the two pH values.

how does titration of a strong monoprotic acid with a strong base differ from a titration...

how does titration of a strong monoprotic acid with a strong base differ from a titration for a weak monoprotic acid with a strong base with respect to the following a) quantity of base required to reach the equivalance point b) ph at the beginning of the titration c) ph at the equivalance point d) ph after addition of a slight access of base e) choice of indicator for determining the equivalence point

Calculate pH for a strong acid/strong base titration. Determine the pH during the titration of 39.8...

Calculate pH for a strong acid/strong base titration. Determine the pH during the titration of 39.8 mL of 0.334 M HI by 0.334 M KOH at the following points: (a) Before the addition of any KOH-? (b) After the addition of 19.9 mL of KOH-? (c) At the equivalence point-? (d) After adding 47.8 mL of KOH-?

Draw a titration curve for both a strong acid titrated by a strong base and a...

Draw a titration curve for both a strong acid titrated by a strong base and a weak acid titrated by a strong base. Identify the equivalence point and the half equivalence point on these graphs. Define each of these points and tell what information these points can give you. Also tell what species are present at the beginning of the titration, at the half equivalence point, at the equivalence point and after the equivalence point. . Draw a titration curve...

Subjects