Describe how to make 2.0L of a 2.00 M solution of sodium carbonate from solid sodium carbonate(s).
b. Describe how you can make a buffer with sodium carbonate(s)
by adding hydrochloric acid.
c. How many mL of 1.00 M HCl(aq) are needed to be added to 10.00 g
of sodium carbonate to make a buffer at pH =10.00. Ka of HCO3- is
4.7 x 10-11.
Ques a) moles of solid sodium carbonate(s) required = 2M x 2L = 4 moles
so, mass of solid sodium carbonate(s) to be mixed in 2 L of solution = 4 x 40= 160 gm
Ques b) when solid sodium carbonate(s) and hydrochloric acid are mixed, then following reaction occurs:
Na2CO3 + HCl --> HCO3- + NaCl
so, here buffer solution of HCO3- /CO3-2 can be made, if after the above reaction, some amount of carbonate anion is left in the solution.
Ques C) 10.00 g of sodium carbonate= 0.25 moles of sodium carbonate= 250 millimoles of sodium carbonate
mL of 1.00 M HCl(aq) be V. So millimoles of HCl used= 1 X V= V millimoles
Na2CO3 + HCl --> HCO3- + NaCl
250-V 0 V
using Henderson–Hasselbalch equation:
PH = Pka + Log([Salt]/[Acid])
10 = 10.3279 + Log([250-V]/[V ])
after simplification, we get V= 170.5 ml
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