Question
In: Chemistry
You make a pH =8 buffer using 100.0 mL of a 1.00 M HClO and solid...
You make a pH =8 buffer using 100.0 mL of a 1.00 M HClO and solid NaClO. You then add 0.0500 mol NaOH (no change in volume). What is the new pH?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
You need to prepare 100.0 mL of a pH = 4.00 buffer solution using 0.100 M...
You need to prepare 100.0 mL of a pH = 4.00 buffer solution
using 0.100 M benzoic acid (pKa = 4.20) and 0.200 M sodium
benzoate. How much of each solution should be mixed to prepare this
buffer?
Calculate the pH of 100.0 mL of a buffer that is 0.0700 M NH4Cl and 0.115 M...
Calculate the pH of 100.0 mL of a buffer that is 0.0700
M NH4Cl and 0.115 M NH3 before and after the addition of
1.00 mL of 5.10 M HNO3.
Before=
After=
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using
0.100 M benzoic acid (pKa = 4.20) and 0.120 M sodium benzoate. How
much of this solution should be mixed to prepare this buffer? Sum
of volumes must equal 100mL. Please explain clearly and show work!
Thank you :)
You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid...
You need to prepare 100.0 mL of a pH=4.00 buffer solution using
0.100 M benzoic acid (pKa = 4.20) and 0.220 M sodium benzoate. How
much of each solution should be mixed to prepare this buffer?
a) mL of benzoic acid
b) mL of sodium benzoate
Calculate the pH of 100.0 mL of a buffer that is 0.0850 M NH4Cl and 0.180...
Calculate the pH of 100.0 mL of a buffer that is 0.0850 M NH4Cl
and 0.180 M NH3 before and after the addition of 1.00 mL of 5.50 M
HNO3.
Can you please do a step-by-step of how to solve this,
paying special attention to how to get the Ka in the Henderson
Hasselbalch Equation? That's the part I'm not
understanding.
Calculate the pH of 100.0 mL of a buffer that is 0.0650 M NH4Cl and 0.185...
Calculate the pH of 100.0 mL of a buffer that is 0.0650 M NH4Cl
and 0.185 M NH3 before and after the addition of 1.00 mL of 5.90 M
HNO3.
Calculate the pH of 100.0 mL of a buffer that is 0.0550 M NH4Cl and 0.180...
Calculate the pH of 100.0 mL of a buffer that is 0.0550
M NH4Cl and 0.180 M NH3 before and after the
addition of 1.00 mL of 5.80 M HNO3.
Calculate the pH of 100.0 mL of a buffer that is 0.060 M NH4Cl and 0.185...
Calculate the pH of 100.0 mL of a buffer that is 0.060 M NH4Cl
and 0.185 M NH3 after the addition of 1.00 mL of 5.00 M HNO3.
Calculate the pH of 100.0 mL of a buffer that is 0.050 M NH4Cl and 0.180...
Calculate the pH of 100.0 mL of a buffer that is 0.050 M NH4Cl
and 0.180 M NH3 before and after the addition of 1.00 mL of 5.70 M
HNO3.
Before =
After=
A 100.0 ml sample of 1.00 M NaOH is mixed with 50.0 ml of 1.00 M...
A 100.0 ml sample of 1.00 M NaOH is mixed with 50.0 ml
of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted
with a lid through which passes a calibrated thermometer. the
temperature of each solution before mixing is 22.9°C. After adding
the NaOH solution to the coffee cup and stirring the mixed
solutions with thermometer; that the specific heat of the mixed
solutions is 4.18 J/(g•°C), and that no heat is lost to the...
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