A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base…
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Question “A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base…”
point.
Weak acid, strong base
Strong acid, strong base
Weak base, strong acid
pH less than 7
pH equal to 7
pH greater than 7
B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH.
Calculate the pH after addition of 28.0 mL of KOH.
C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5)
with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the
titrant.
D. A 30.0 mL volume of 0.50 M CH3COOH (Ka = 1.8 x 10^-5) was
titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0
mL of NaOH.
Answer
Based on their pH value, solutions can be classified as acids or bases.
Titration refers to a method where a concentrated solution of a known substance is used to determine the concentration of an unknown solution. The solution to a known concentration is known as a titrant, while the solution to an unknown concentrated is known as an analyte.
pH is a measurement of the hydrogen ion in a solution. It is the negative logarithm for the H + concentration to base 10. It is the acidic strength of a solution.
Acid: acid substance can accept or donate a proton.
Basis:Base substance can either accept a proton, or give two electrons.
Based on their pH value, solutions can be classified as acids or bases. The pH value of a solution determines whether it is acidic or basic. pH values less than 7 are considered acidic. pH values greater than 7 are considered to be basic.
pH can be determined by measuring the concentration of

within the solution.

value is negative logarithm (base

) of the Hydrogen ion concentration
![[н]](https://drive.google.com/uc?id=1n2UsMiQVcx9X99QOFTs77-L5nAz9Rz9b&export=download/A.-Match-each-type-of-titration-to-its-pH-at-the-equivalence-point.-Weak-acid,-strong-base-Strong-acid,-strong-base.png?x-oss-process=image/resize,w_560/format,webp)
.

Molarity: Mole is the ratio between the solution’s volume and the number of moles.



refers to the equilibrium reaction’s base dissociation and ionization constant.

is the expression for the equilibrium reaction.
![ОН + B*
ВОН
Гон Тв]
К
[Вн]](https://drive.google.com/uc?id=1uZo17eYBxmMi1CZnDrKkGA65V-R-6Aoo&export=download/A.-Match-each-type-of-titration-to-its-pH-at-the-equivalence-point.-Weak-acid,-strong-base-Strong-acid,-strong-base.png?x-oss-process=image/resize,w_560/format,webp)

refers to the expression of an acid dissociation constant or ionization factor for equilibrium reactions.

is the expression for an equilibrium reaction.

(A)

(B)





(C)











![[H]
pH= -log (*)
pH log
7.48x10
= 5.13](https://drive.google.com/uc?id=1dvBiWwjhAnogxNGez8SIyDFsS3adYUX8&export=download/A.-Match-each-type-of-titration-to-its-pH-at-the-equivalence-point.-Weak-acid,-strong-base-Strong-acid,-strong-base.png?x-oss-process=image/resize,w_560/format,webp)
Ans Part A

Conclusion
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