A buffer solution is made that is 0.480 M in H2S and 0.480 M in NaHS. If Kal for H2S is 1.00 × 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.129 mol HBr is added to 1.00 L of the buffer sol (Use the lowest possible coefficients. Omit states of matter. Use H3 O* instead of H+) +

A buffer solution is made that is 0.480 M in H2S and 0.480 M in NaHS. If Kal for H2S is 1.00 × 10-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.129 mol HBr is added to 1.00 L of the buffer sol (Use the lowest possible coefficients. Omit states of matter. Use H3 O* instead of H+) +

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

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Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
A buffer solution is made that is 0.496 M in H2S and 0.496 M in NaHS . If Ka1 for H2S is 1.00 x 10^-7 , what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.131 mol HI is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O^+ instead of H^+ ) + +
A buffer solution is made that is 0.394 M in H2S and 0.394 M in NaHS. If Ka1 for H2S is 1.00 x 10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.098 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use instead of )
1) In the laboratory, a general chemistry student measured the pH of a 0.554 M aqueous solution of nitrous acid to be 1.787. Use this information she obtained to determine the Ka for this acid? Ka .......................... ? 2) How many grams of solid potassium hydroxide ( molar mass= 56.1 g/mol) are needed to react with 26.7 mL of a 1.75 M hydroiodic acid solution? KOH + HI......> kI + H2o ................ grams
1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?
A chemist starts her experiments with 25.00 mL of 0.125 mol L-1 NaCN solution. The pKa of HCN = 9.20. a) What volume of 0.100 mol L-1 HCl will be required to fully react with the above salt? b) After the reaction in part (a) takes place, will the pH of the solution be acidic, basic or neutral? c) What volume of 0.100 mol L-1 HCl is needed to adjust the pH of the originally provided solution to pH = 9.00? HINT: At pH 9.00, what kind of solution is created if the pKa of HCN is 9.20
A buffer is prepared by dissolving 0.80 moles of NH3 and 0.80 moles of NH4Cl in 1.00 L of aqueous solution. If 0.10 mol of NaOH is added to 250 mL of this buffer, what is the pH of the resultant solution? Kb of NH3 = 1.8 x 10–5
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