Can you help me with number 28 27282930Which of the following buffer solutions will bestprotect around a pH of 11.0?Assume all chemicals are 1.0M in solutionWhat is the final pH when a solution is made thatcontains 0.250M HNO₂ and 0.450M KNO₂2Ka HNO₂ = 7.2*10-4WWhat is the final pH when a buffer contains 1.00mol of CH3NH2 and 2.00 mol of CH3NHst. 0.750mol of NaOH is added to the solution. Assumingno dilution, what is the final pH of the solution?CH3NH2 Kb = 4.3*10-4.100 moles of HCI is added to a 1L mixture of100M HC3HsO2 and 0.180M KC3H5O2. Assumingno volume change, what will be the final pH in thesolution?Ka HC3H5O2 4.5*10-5>TimIl Proctoric

Concentration of HNO2 = 0.250 MConcentration of KNO2 = 0.450 MKa of HNO2 = 7.2×10-4

Answered: 28 What is the final pH when a solution…

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28 What is the final pH when a solution is made that contains 0.250M HNO₂ and 0.450M KNO₂ Ka HNO₂ = 7.2*10-4 >

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Can you help me with number 28

27
28
29
30
Which of the following buffer solutions will best
protect around a pH of 11.0?
Assume all chemicals are 1.0M in solution
What is the final pH when a solution is made that
contains 0.250M HNO₂ and 0.450M KNO₂2
Ka HNO₂ = 7.2*10-4
W
What is the final pH when a buffer contains 1.00
mol of CH3NH2 and 2.00 mol of CH3NHst. 0.750
mol of NaOH is added to the solution. Assuming
no dilution, what is the final pH of the solution?
CH3NH2 Kb = 4.3*10-4
.100 moles of HCI is added to a 1L mixture of
100M HC3HsO2 and 0.180M KC3H5O2. Assuming
no volume change, what will be the final pH in the
solution?
Ka HC3H5O2 4.5*10-5
>
Tim
Il Proctoric

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