A solution was composed of 50.0 mL of 0.1 M C6H8O6and50.0 mL0.100M NaC6H7O6. a. Would this solution act as a buffer? Explain your answer. Ka is 6.3 X10^-5 b. How might the solution’s pH change if 10.0 mL of 0.100MNaOH were added to it?

A chemistry graduate student is given 250. mL of a 0.30M chloroacetic acid (HCH,CICO,) solution. Chloroacetic acid is a weak acid with K= 1.3 × 10 °. What mass of KCH,CICO, should the student dissolve in the HCH,CICO, solution to turn it into a buffer with pH = 2.80? You may assume that the volume of the solution doesn't change when the KCH,CICO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

Write the titration reaction of 100 mL of 0.100 M anilinium bromide (“aminobenzene . HBr”) +.100 M NaOH.

A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system.   Choices:  HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol)  NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)

What quantity in moles of CH₃NH₃Cl  need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 11.00?

What quantity in moles of CH₃NH₃Cl  need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 10.90?

A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.

A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x10

What concentration of each form (deprotonated and protonated) of this buffer would you need to create 500mL of a 0.02M MOPS buffer that has a pH equal to 7.5?

A buffer is made using 100.0 mL of 0.100 M CH3CH2COOH (propanoic acid) and 100.0 mL of 0.100 M NaCH3CH2COO (sodium propanoate). 10.0 mL of 0.100 M HCl is added to the buffer. What is the solution pH after the HCl is added?For CH3CH2COOH K = 1.3 x 10^-5