The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a) HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq). b) How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq)?
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The pH of a 1.00 M NaCH3COO (aq) solution is 9.38.
a) HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the
b) How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq)?
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- Calculate the change in pH when 5.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). A list of ionization constants can be found here. B)Calculate the change in pH when 5.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.Calculate the change in pH when 3.00 mL3.00 mL of 0.100 M HCl(aq)0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq)NH3(aq) and 0.100 M in NH4Cl(aq).NH4Cl(aq). Consult the table of ionization constants as needed. Calculate the change in pH when 3.00 mL3.00 mL of 0.100 M HCl(aq)0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq)NH3(aq) and 0.100 M in NH4Cl(aq).NH4Cl(aq). Consult the table of ionization constants as needed. Calculate the change in pH when 3.00 mL3.00 mL of 0.100 M NaOH0.100 M NaOH is added to the original buffer solution. Calculate the change in pH when 3.00 mL3.00 mL of 0.100 M NaOH0.100 M NaOH is added to the original buffer solution..Which statement describes the action of a buffer composed of acetic acid (CH3COOH) and sodium acetate (NaCH3COO)? How does a buffer resist change in pH upon addition of a strong acid? By titration, it is found that 73.3 mL of 0.189 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Consult the table of ionization constants as needed. Then, Calculate the change in pH when 8.00 mL of 0.100 M NaOH is added to the original buffer solution.A solution is prepared by adding 100 mL of 1.0 M HC,H,O,(aq) to 100 mL of 1.0 M NaC,H,O,(aq). The solution is stirred and its pH is measured to be 4.73. After 3 drops of 1.0 M HCl are added to the solution, the ph of the solution is measured and is still 4.73. Which of the following equations represents the chemical reaction that accounts for the fact that acid was added but there was no detectable change in pH? (A) H;O*(aq) + OH (aq) → 2 H,O(1) (B) H;O*(aq) + CI (aq) → HCI(g) + H,O(1) (C) H,O*(aq) + C,H,O, (aq) → HC,H,0,(aq) + H,0(1) (D) H;O*(aq) + HC,H,O,(aq) - H,C,H,0,*(aq) + H,O()An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of 1.0 L. What is the effect of adding 0.50 mol CH3CO2–(aq) to this solution? 1.The pH of the solution will equal 7.00 because equal concentrations of a weak acid and its conjugate base are present. 2.Some CH3CO2H(aq) will ionize, increasing the concentration of CH3CO2–(aq) and increasing the pH.3.Some CH3CO2–(aq) will react with H3O+, increasing the concentration of CH3CO2H(aq) and reestablishing the solution equilibrium. b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3
- Calculate the change in pH when 8.00 mL of .100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Consult the table of ionization constants as needed. ΔpH= Calculate the change in pH when 8.00 mL of 0.100 M NaOH is added to the original buffer solution. ΔpH= The last person to help me on here got it wrong so please help me to understand how to do itThe reaction of the weak acid HCN with the strong base KOH is HCN(aq) + KOH(aq) HOH(l) + KCN(aq) To compute the pH of the resulting solution if 63 mL of 0.88 M HCN is mixed with 32 mL of 0.34 KOH, we need to start with the stoichiometry. Let us do just the stoichiometry in steps. How many moles of acid? How many moles of base? What is the limiting reactant? How many moles of the excess reactant after reaction? What is the concentration of the excess reactant after reaction? What is the concentration of the pH active product after reaction? number of moles: number of moles: limiting reactant: number of moles: concentration: concentration:2.500 g of an unknown achiral primary amine is dissolved in enough water to yield a 50.00 mL solution. This solution is titrated with 0.9250 M HCl(aq). After 24.95 mL of titrant is added, the pH of the resulting solution is 10.28. After a total of 36.95 mL of titrant is added, the equivalence point is reached. Calculate the molar mass (MM) of the unknown amine.
- Propionic acid, HC3H5O2, has a Ką value of 1.3 x 105. A buffer solution is prepared by mixing 20.0 mL of 0.100 M HC3H5O2(aq) with 10.0 mL of 0.100 M NaC3H502(aq), its conjugate base. The pH of this buffer solution is measured to be 4.59. What is the concentration (in M) of the acidic component of this buffer solution. Express your answer to 3 significant figures, using theCalculate the pH for each case in the titration of 50.0 mL of 0.220 M HClO(aq)0.220 M HClO(aq) with 0.220 M KOH(aq).0.220 M KOH(aq). Use the ionization constant for HClO.Calculate the change in pH when 9.00 of 0.100 M HCl * (aq) is added to 100.0 of a buffer solution that is 0.100 M NH 3 (aq) and 0.100 M in NH 4 Cl(aq) . Consult the table of ionization constants as needed. Delta*p * H = Calculate the change in pH when 9.00 mL of 0.100 M NaOH is added to the original buffer solution. Delta*p * H =