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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Calculate the pH of a buffer solution made by dissolving 50.0 g of NaHCO3 and 20.0 g H2CO3 to make 100 mL of a buffer solution. H2CO3= Ka1= 4.30 x 10^7
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- A buffer solution is made that is 0.409 M H2S and 0.409 M in NaHS. If Ka1 for H2S is 1.00x10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.087 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)arrow_forwardA student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.14 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. During the titration the following reaction occurs HA + NaOH ⇒ NaA + H2OWhat is the concentration of A- (the conjugate base of the weak acid) at the equivalence point? ml NaOH added pH Hal-way point 18.71 3.41 Equivalence point 37.41 8.53arrow_forwardCalculate the pH of a buffer solution prepared by dissolving 0.400 mol of cyanic acid (HCNO) and 0.800 mol of sodium cyanate (NACNO ) in enough water to make 1.00 L of solution. The Ka of HCNO at 25° C is 2.00 x 10-4arrow_forward
- 20. mL of 0.250 M NH3 is titrated with 0.500 M of HCl solution, what is the pH of the resulting solution when 0mL, 5.0 mL, 10.0 mL and 12 mL of HCl was added into the NH3solution? KB(NH3) = 1.8 x 10-5arrow_forwardJust as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, - log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L-' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kh for ammonia is 1.8 × 10–5. pKa base] pH = pKa +log acid Express your answer to two significant figures and include the appropriate units. Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. • View Available Hint(s) ? X•10n Value mass of NHẠCI = Unitsarrow_forwardAn analytical chemist is titrating 64.8mL of a 0.3000M solution of ammonia NH3 with a 0.7300M solution of HNO3 . The pKb of ammonia is 4.74 . Calculate the pH of the base solution after the chemist has added 31.6mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.arrow_forward
- Calculate the pH of a buffered solution that is 0.100 M in C6H5COOH (Ka = 6.4 x 10–5) and 0.100 M in C6H5COONaarrow_forwardCalculate the pH of a titration solution formed when 45.0 mL of 0.100 M NaOH is added to50.0 mL of 0.100 M CH3COOH (Ka = 1.8×10-5).arrow_forward8. You will perform some calculations to see the difference between a pH buffer solution and a weak acid solution of the same pH when a small amount of strong base is added. Chlorous acid, HC1O₂, is a moderately strong acid with a Ka = 1.110×10-². Please answer the following questions. A. B. What is the molarity of the HClO₂ solution whose pH is 2.21? Please provider your answer below. 미ㄷ → Please provider your answer below. f A $ To prepare a buffer solution of the same pH, what is the molarity of the NaClO₂ if the molarity of the HC1O₂ is 0.6771 M? M → M → $arrow_forward
- If a buffer solution is 0.180 M in a weak acid (Ka = 1.7 × 10 − 5 ) and 0.600 M in its conjugate base, what is the pH?arrow_forwardCalculate the pH of a buffer made by adding HCO2H (formic acid) and NaCOH to water if at equilibrium [CO2H'] = 8.00 x 10-3 M, [HCO2H] = 2.50 x 104 M, and the Ka = 1.77 x 104. This is part 1, give the [H3O*l] HCO2H + H20 e CO2H1 + H30+1 A. 2.21 x 102 B. 4.43 x 10-8 C. 1.81 x 105 D. 5.53 x 10-6arrow_forwardCalculate the pH of a solution at the equivalence point when 200.0 mL of a 0.20 M solution of acetic acid (HC3H5O3), which has a Ka value of 1.4 x 10–4, is titrated with a 0.10 M LiOH solution.arrow_forward
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