If a solution of glycine has a pH of 1.88, the initial concentration of thethe glycine solution is a.b * 10c mol/L. The values of a, b and c are ______, ______ and ______.
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b) In a 0.1M solution of glycine at pH 9.0, what fraction of glycine has its amino group in the -NH3+ form? c) How much 5M KOH must be added to 1.0L of 0.1M glycine at pH 9.0 to bring its pH to exactly 10.0? d) When 99% of the glycine is in its -NH3+ form, what is the numerical relation between the pH of the solution and the pKa of the amino group?
Sri K.
What is the $\mathrm{pH}$ of $0.01 \mathrm{M}$ glycine solution? For glycine $\mathrm{Ka}_{1}=4.5 \times 10^{-3}$ and $\mathrm{Ka}_{2}=1.7 \times 10^{-10}$ at $298 \mathrm{~K}$ a. $6.94$ b. $7.06$ c. $5.06$ d. $8.02$
Three acidic solutions A, B and C have pH = 1, 3 and 5 respectively: (i) Which solution has the highest concentration of H+ ions? (ii) Which solution has the lowest concentration of H+ ions?
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