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If you added 4.5ml of 1.0M HCI to 100ml of 0.10M glycine, pH 12.0, what would be the expected (calculated) pH?Note: Assume that at a pH of 12.0, there are 9.96mmol of the base form (NH2) of glycine in solution. The pKa of basic amine functional group (NH2) in glycine = 9.6 and the pKa of the acidic carboxyl group in() = 2.3.

Name: if you added 45ml of 10m hci to 100ml of 010m glycine ph 120 what would be the expected calculated phnote assume that at a ph of 120 there are 996mmol of the base form nh2 of glycine in solu 70074
Uploaded: 2023-06-14T18:36:41-08:00
Duration: 3 min 3 s
Channel: Nicholas Mogoi
Description: if you added 45ml of 10m hci to 100ml of 010m glycine ph 120 what would be the expected calculated phnote assume that at a ph of 120 there are 996mmol of the base form nh2 of glycine in solu 70074

          If you added 4.5ml of 1.0M HCI to 100ml of 0.10M glycine, pH 12.0, what would be the expected (calculated) pH?Note: Assume that at a pH of 12.0, there are 9.96mmol of the base form (NH2) of glycine in solution. The pKa of basic amine functional group (NH2) in glycine = 9.6 and the pKa of the acidic carboxyl group in() = 2.3.

Added by Brian B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Nicholas Mogoi

06/14/2023

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0 \text{ M} \times 4.5 \times 10^{-3} \text{ L} = 4.5 \times 10^{-3} \text{ mol} \] Show more…

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If you added 4.5ml of 1.0M HCI to 100ml of 0.10M glycine, pH 12.0, what would be the expected (calculated) pH?Note: Assume that at a pH of 12.0, there are 9.96mmol of the base form (NH2) of glycine in solution. The pKa of basic amine functional group (NH2) in glycine = 9.6 and the pKa of the acidic carboxyl group in() = 2.3.