Which of the following aqueous mixtures would be a buffer system? A) HCI, NaCl B) HNO3, NaNO3 C) H3PO4, NaH2PO4 D) H2SO4, CH3COOH E) NH3, NaOH Which solution is a buffer? A) a solution that is 0.100 M in HNO2 and 0.100 M in HC1 B) a solution that is 0.100 M in HNO3 and 0.100 M in NaNO3 C) a solution that is 0.100 M in HNO2 and 0.100 M in NaCl D) a solution that is 0.100 M in HNO3 and 0.100 M in NAOH E) a solution that is 0.100 M in HNO2 and 0.100 M in NANO2

Which of the following aqueous mixtures would be a buffer system? A) HCI, NaCl B) HNO3, NaNO3 C) H3PO4, NaH2PO4 D) H2SO4, CH3COOH E) NH3, NaOH Which solution is a buffer? A) a solution that is 0.100 M in HNO2 and 0.100 M in HC1 B) a solution that is 0.100 M in HNO3 and 0.100 M in NaNO3 C) a solution that is 0.100 M in HNO2 and 0.100 M in NaCl D) a solution that is 0.100 M in HNO3 and 0.100 M in NAOH E) a solution that is 0.100 M in HNO2 and 0.100 M in NANO2

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 61QAP: Each symbol in the box below represents a mole of a component in one liter of a buffer solution;...

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Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
How many 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? Let x represent the original concentration of CH3COO- in the water. Based on the given values, set up the ICE table in order to dtermine the unknown.
Which of these statements is true? (a) If you add strong acidor base to a buffer, the pH will never change. (b) In orderto do calculations in which strong acid or base is added toa buffer, you only need to use the Henderson–Hasselbalchequation. (c) Strong bases react with strong acids, but not weak acids. (d) If you add a strong acid or base to a buffer, thebuffer’s pKa or pKb will change. (e) In order to do calculationsin which a strong acid or base is added to a buffer, you need tocalculate the amounts of substances from the neutralizationreaction and then equilibrate.
Student Q prepared 50.0 mL of a buffer solution using 0.50 moles of HA and 0.50 moles of A- while Students S prepared 50.0 mL of a buffer using 0.25 moles of HA and 0.25 mole of A-. a. Do the two buffer solutions have the same or different pH? Explain b. If 1.00mL of 0.010M NaOH were added to the two buffers, would the pH of the two solutions increase or decrease? Explain. c. Which solution (Buffer Q or Buffer S) would show a smaller chanign in pH for question b? Explain.
An aqueous solution contains 0.399 M dimethylamine ((CH3)2NH).How many mL of 0.369 M hydrochloric acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.500? (answer is 110 mL)
Calculate the [H3O*] of 114.01 mL of a buffer initially consisting of 0.1752 M C2H5NH2 and 0.1926 M C2H5NH3Br after addition of 0.0031 mol of HCI Assume that no volume change occurs after addition of the acid. The Kb of C2H5NH2 is 5.60e-4
What volume, in milliliters, of 0.210 M NaOH should be added to a 0.125 L solution of 0.025 M glycine hydrochloride (p?a1=2.350, p?a2 = 9.778) to adjust the pH to 2.61? Please explain. Please type answer note write by hend.
A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated
For 280.0 mL of a buffer solution that is 0.315 M in CH3CH2NH2 and 0.220 M in CH3CH2NH3Cl, calculate the initial pH and the final pHpH after adding 0.024 mol of NaOH. ( Kb(CH3CH2NH2)=5.6×10−4Kb(CH3CH2NH2)=5.6×10−4.)
How many moles of sodium hydroxide would have to be added to 150 mL of a 0.417 M nitrous acid solution, in order to prepare a buffer with a pH of 3.260? I want handwritten solution....i will up vote