CW13-Buf - M NH 4 Cl. (a) What concentrations would exist...

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CHM 2046/Myers Worksheet 13 February 9 or 11, 2010 1. Review – The 5 Problem Types in Acid-Base Chemistry : SA WA Buffer WB SB 2. A solution is both 0.10 M NH 3 and 0.20 M NH 4 Cl. The concentrations are : [NH 3 ] = ___________ [NH 4 + ] = [Cl - ] = ______________ What is the pH of this buffer? pH = ______________ 3. A solution is prepared by mixing 200. mL of 0.40 M NH 3 and 100. mL of 0.30 M NH 4 Cl. Now what are the principal specie concentrations . (There is no reaction here, but each solution dilutes the other .) [NH 3 ] = ______________ [NH 4 + ] = [Cl - ] = ______________ What is the pH of this buffer? pH = ______________
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4. A solution is prepared by mixing 400. mL of 0.10 M NaOH and 100. mL of 0.50
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Unformatted text preview: M NH 4 Cl. (a) What concentrations would exist after mixing but before any reaction ? [Na+] = [OH-] = ______________ [NH 4 + ] = [Cl-] = ______________ (b) What appreciable concentrations will exist after reaction to completion ? OH-+ NH 4 + H 2 O + NH 3 [Na + ] = _______________ [Cl-] = ________________ [______] = ______________ [NH 3 ] = _______________ What is the pH of this final solution? pH = ______________ 5. When do you do an ICC type calculation? When ICE?...
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This note was uploaded on 09/19/2011 for the course CHM 2051 taught by Professor Staff during the Spring '08 term at University of Florida.

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CW13-Buf - M NH 4 Cl. (a) What concentrations would exist...

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