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13 Dec 2019

Calculate the number of moles & grams of ammonium chloride (NH4CL) used to prepare a buffer of volume 500ml that is 0.1M ammonia (NH3). Kb NH3 = 1.8 x 10-5 and pH = 9.15

I'm good with the basic Henderson-Hasselbalch Equation, but I'm not sure how to formulate this data to get the answer. Thanks for any assistance.

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Jean Keeling
Jean KeelingLv2
17 Dec 2019

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Related questions

Please PLease help!

Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka,

pKa=−logKa

The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions:
pH=pKa+log[base][acid]

Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and pKb is similar.

pOH=pKb+log[acid][base]

1.) How many grams of dry NH4Cl need to be added to 2.00 L of a 0.600 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.61? Kb for ammonia is 1.8×10−5.

Express your answer with the appropriate units.

How many grams of dry NH4Cl need to be added to 2.40 L of a 0.100 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.52? Kb for ammonia is 1.8×10−5.

Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka,

pKa=−logKa

The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions:

pH=pKa+log[base]/[acid]

Notice that the pH of a buffer has a value close to the pKaof the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and pKb is similar.

pOH=pKb+log[acid]/[base]

best answer will be rated. Thank you for your time in advance!!

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