prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and concentrated NH4OH ,...

prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and concentrated NH4OH , the NH4OH molartiy is 18.1 M ? NH4OH is equal to NH3 (aq)

Expert Solution

PH = 10

POH = 14-PH

= 14-10 = 4

[NH3] = 18.1M

POH = Pkb + log[NH4Cl]/[NH3]

4 = 4.75 + log[NH4Cl]/18.1

4-4.75 = log[NH4Cl]/18.1

log[NH4Cl]/18.1 = -0.75

[NH4Cl]/18.1 = 10^-0.75

[NH4Cl]/18.1 = 0.178

[NH4Cl] = 0.178*18.1 = 3.2218M

no of moles of NH4Cl = molarity * volume in L

= 3.2218*0.1 = 0.32218moles

mass of NH4Cl = no of moles * gram molar mass

= 0.32218*53.5 = 17.24g

queen_honey_blossom answered 2 years ago

calculate the pH of 100 mL of a buffer that is .080 M NH4Cl and .105...

calculate the pH of 100 mL of a buffer that is .080 M NH4Cl and .105 M NH3 before and after the addition of 1.00mL of 6.05 M HNO3

You are to prepare 100 mL of a pH 3.76 buffer solution with a formal concentration...

You are to prepare 100 mL of a pH 3.76 buffer solution with a formal concentration of 0.0500 F (i.e., total concentration of all acetate species is 0.0500 M). Calculate how many grams, of acetic acid and sodium acetate mix together.

How many moles of NH4Cl must be added to 100 mL of 0.1 M NH4OH solution...

How many moles of NH4Cl must be added to 100 mL of 0.1 M NH4OH solution to prevent precipitation of Mn(OH)2 when this solution is added to 100 mL of a 0.002 M solution of MnCl2? Assume no change involume on addition of NH4Cl.

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 0.0850 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=

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 :)

Question