Question
In: Chemistry
A 30.00 mL sample of 0.200 M HBr was titrated with 0.160 M KOH. a. What...
A 30.00 mL sample of 0.200 M HBr was titrated with 0.160 M KOH.
a. What is the initial pH of the sample?
b. What is the equivalence volume?
c. What is the pH after 19.16 mL of KOH is added?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Consider the titration of a 34.0 mL sample of 0.170 M HBr with 0.200 M KOH....
Consider the titration of a 34.0 mL sample of 0.170 M HBr with
0.200 M KOH. Determine each of the following:
1. initial pH
2. the volume of added base required to reach the equivalence
point
3. pH at 10.4 mL of added base
4. pH at the equivalence point
2) A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M HCl. Determine...
2)
A 25.0 mL sample of 0.160 M KOH is titrated with 0.250 M
HCl.
Determine the following quantities:
a)
The initial pH of the KOH solution before any acid is added.
b)
The pH of the solution after 3.00 mL of HCl is added.
c)
The quantity of HCl solution required to reach the
equivalence
point.
d)
The pH of the solution at the equivalence point.
e)
The pH of the solution after20.0 mL of HCl is added.
A 40.0-mL sample of 0.100 M HNO2 is titrated with 0.200 M KOH. Calculate: a.the volume...
A 40.0-mL sample of 0.100 M HNO2 is titrated with 0.200 M KOH.
Calculate:
a.the volume required to reach the equivalence point
b.the pH after adding 15.00 mL of KOH
c.the pH at one-half the equivalence point
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
A) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the...
A) A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH.
Calculate the pH after the addition of 20.0 mL of KOH.
B) A 75.0-mL volume of 0.200 M NH3
(Kb=1.8×10−5) is titrated with 0.500 M HNO3.
Calculate the pH after the addition of 28.0 mL of HNO3.
C) A 52.0-mL volume of 0.35 M CH3COOH
(Ka=1.8×10−5) is titrated with 0.40 M NaOH.
Calculate the pH after the addition of 15.0 mL of NaOH.
For all of the following questions 20.00 mL of 0.195 M HBr is titrated with 0.200...
For all of the following questions 20.00 mL of 0.195 M HBr is
titrated with 0.200 M KOH.
Region 1: Initial pH: Before any titrant is added to our starting
material
What is the concentration of H+ at this point in the
titration?
M
What is the pH based on this H+ ion concentration?
Region 2: Before the Equivalence Point 5.68 mL of the 0.200 M KOH
has been added to the starting material.
Complete the BCA table below at...
A 625 mL solution of HBr is titrated with 1.51 M KOH. If it takes 728.5...
A 625 mL solution of HBr is titrated with 1.51 M KOH. If it
takes 728.5 mL of the base solution to reach the equivalence point,
what is the pH when only 137 mL of the base has been added to the
solution?
I am getting an answer of .1018, but it's wrong
partb a)A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the...
partb a)A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M
KOH. Calculate the pH after the addition of 13.0 mL of KOH. Express
your answer numerically. Part b) A 75.0-mL volume of 0.200 M NH3
(Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after
the addition of 15.0 mL of HNO3. Express your answer
numerically.Part c) A 52.0-mL volume of 0.35 M CH3COOH
(Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after
the...
30.0 mL of 0.100 M H2CO3 is titrated with 0.200 M KOH. Calculate the initial pH...
30.0 mL of 0.100 M H2CO3 is titrated with 0.200 M KOH. Calculate
the initial pH before KOH has been added. ka = 4.3 x 10-7.
Calculate the pH when 10.0 mL of a .200M KOH is added to 30.0 mL of
0.100 M H2CO3. ka = 4.3 x 10-7. Calculate the equivalence point and
then calculate the pH at the equivalence point. Calculate the pH if
20.0 mL of 0.200 M KOH is added to 30.0 mL of 0.100...
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- Singh Development Co. is deciding whether to proceed with Project X. The cost would be $12...
- CS2123 Data Structures - Fall 2019 Assignment 1: Function Runtimes Table Due 9/11/19 by 11:59pm Completing...
- Question 2. Design a 16-1 MUX using any number of lower MUXs, such as 8-1 or...
- . Write a function that takes, as arguments, two objects, value1 and value2. If
- Wii Brothers, a game manufacturer, has a new idea for an adventure game. It can market...
- Consider the distillation of ethanol (C2H5OH) and the combustion of ethanol . Use a bullet point...
- 1.How does Economic exposure to exchange rate movements affect the capital budgeting of a firm? Provide...
ADVERTISEMENT