Calculate the pH of a buffer solution composed of 0.15M HF and 0.15M NaF. Ka for HF is 6.8 x 10-4. Calculate the ΔpH caused by the addition of 7.0 ml of 0.10M NaOH to 100ml of the buffer solution obtained in part (a).
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Calculate the pH of a buffer solution composed of 0.15M HF and 0.15M NaF. Ka for HF is 6.8 x 10-4.
Calculate the ΔpH caused by the addition of 7.0 ml of 0.10M NaOH to 100ml of the buffer solution obtained in part (a).
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- Calculate the change in pH when 6.00 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. ΔpH=? Calculate the change in pH when 6.00 mL of 0.100 M NaOH is added to the original buffer solution. ΔpH=?Consider a flask containing 25.00 mL of 0.100M sodium benzoate (NaC, H5C00). This is titrated with a 0.110 M nitric acid solution from a burette. Given: K, of C,H;co0" is 1.6 x 10-10. Determine the pH of the solution in the flask after 32.00 mL of the acid has been added? You must show any reaction equation(s) that you may think are necessary. Determine the pH of the solution in the flask at the half-way point of the titration.(a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer. What is the pH of the buffer after the addition of 0.030 mol HCl? note: Ka (NH4+) = 5.6 x 10 -10 NH3 (aq) + H+ (aq) → NH4+ (aq) (b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.
- Consider the titration of a weak acid that has a pKa = 4.00. Suppose a chemist was going to perform a titration on 50.0 mL of 0.050 0 M of the weak acid using 0.500 M NaOH. (A) What would be the pH of the solution after 0.00 mL of 0.500 M NaOH has been added?(B) What would be the pH halfway to the equivalence point of the titration?(C) What would be the pH at the equivalence point in the titration? (D) What would be the pH of the solution after 6.00 mL of 0.500 M NaOH has been added? Use the following reasoning when solving this problem. Because at the equivalence point the moles of strong base (0.500 M NaOH) added as a titrant equal the moles of weak acid, HA (50.0 ml of 0.050 M) in the solution, we can start by calculating the volume of 0.500 M NaOH needed to reach the equivalence point. To do this we simply equate the moles of HA to moles of NaOH by using the dilution formula. i.e. MaVa = MbVb where a represents HA and b represents NaOH. To calculate volume of NaOH needed to reach…Consider a buffer solution containing 0.040 M ammonia (NH3) and 0.060 M ammonium chloride (NH4Cl). What is the pH of the resulting buffer solution after adding 5.0 mL of 1.0 M sodium hydroxide (NaOH) to 1 L of this buffer? Assume that the volume change upon addition of sodium hydroxide into the buffer is not significant. The Ka of NH4+ is 5.70 x 10-10.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.
- Given that Ka's for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 x 10-4 and 5.4 x 10-10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers. Find the pH of (a) 0.100 M HClO and 0.100 M NaClO; (b) 0.100 M HClO and 0.150 M NaClO; (c) 0.150 M HClO and 0.100 M NaClO; (d) 1.0 L of the solution in part (a) after 0.0050 mol of NaOH has been added.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 it
- Two solutions of an unknown slightly soluble salt, A(OH)2, were allowed to equilibrate—one at 25 °C and the other at 80 °C. A 15.00 mL aliquot of each solution is titrated with 0.200 M HCl. 6.37 mL of the acid is required to reach the endpoint of the titration at 25 °C, while 62.60 mL are required for the 80 °C solution. Assuming that the change in enthalpy is negligible over this temperature range, calculate ΔHCalculate the pH of a buffer system containing 1.0 M CH3COOH and 1.2 M CH3COONA. The Ka for the acid is 1.8 x 10s.Calculate the pH of a buffer formed by mixing 85.0 mL of 0.130 M lactic acid, HC3H5O3, with 95.0 mL of a 0.150 M solution of sodium lactate, NaC3H5O3. The Ka of lactic acid is 1.40 x 10-4.