1) A buffer can be prepared by mixing two solutions. Determine if each of the following…
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1) A buffer can be prepared by mixing two solutions. Determine if each of the following…
1)
A buffer can be prepared by mixing two solutions. Determine if each of the following mixtures will result in a buffer solution or not.
1) Mixing 100.0 mL of 0.1 M HCl with 100.0 mL of 0.1 M NaOH [ Select ] [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]
2) Mixing 100.0 mL of 0.1 M CH3COOH with 100.0 mL of 0.05 M mol CH3COONa [ Select ] [“Yes, it will result in a buffer solution.”, “No, it will not result in a buffer solution.”]
3) Mixing 100.0 mL of 0.1 M NH3 with 100.0 mL of 0.1 M NH4Cl [ Select ] [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]
4) Mixing 100.0 mL of 0.1 M NH3 with 100.0 mL of 0.05 M HNO3 [ Select ] [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]
5) Mixing 100.0 mL of 0.1 M NH3 with 100.0 mL of 0.1 M HNO3 [ Select ] [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]
2) A 1.0 L solution initially contains 0.2 M CH3COOH. Approximate the number of moles of CH3COOH and CH3COO− in the solution after 0.1 mol of solid NaOH is added, and calculate the pH of the resulting solution. Ka of CH3COOH is 1.8
×10−5.
1) The number of moles of CH3COOH present is [ Select ] [“0.0”, “0.2”, “0.1”] mol.
2) The number of moles of CH3COO− present is [ Select ] [“0.1”, “0.0”, “0.2”] mol.
3) The pH of the resulting solution is [ Select ] [“4.44”, “4.74”, “5.05”] .
