Which solution is a buffer? O A solution made from 50.0 mL of 0.100M HNO, and. 50.0 mL of of 0.025 M NaOH O A solution made from 50.0 mL of 0.100 HCl and 50.0 mL of 0.025 M NaNO3 O A solution made from 50.0 mL of 0.100 M H2SO, and 50.0 mL of 0.025 M Na SO4 O A solution made from 50.0 mL of 0.100 M HNO, and 50.0 mL of 0.025 M NaNO3

Which solution is a buffer? O A solution made from 50.0 mL of 0.100M HNO, and. 50.0 mL of of 0.025 M NaOH O A solution made from 50.0 mL of 0.100 HCl and 50.0 mL of 0.025 M NaNO3 O A solution made from 50.0 mL of 0.100 M H2SO, and 50.0 mL of 0.025 M Na SO4 O A solution made from 50.0 mL of 0.100 M HNO, and 50.0 mL of 0.025 M NaNO3

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.30QAP

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Similar questions

. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. Use 1.80105 as Ka for acetic acid. (a) What is the pH of the solution? (b) Is the solution acidic or basic? (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of the original buffer?
Explain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
. Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.
There is a buffer system in blood H2PO4 HPO42 that helps keep the blood pH at 7.40. (K aH2PO4 =6.2108). (a) Calculate the[ H2PO4 ]/[ HPO42 ] ratio at the normal pH of blood. (b) What percentage of the HPO42 ions are converted to H2PO4 when the pH is 7.00? (c) What percentage of the H2PO4ions are converted to HPO42 when the pH is 8.00?
Mixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain. How does the amount of each solution added change the effectiveness of the buffer?
Blood is buffered mainly by the HCO3 H2CO3 buffer system. The normal pH of blood is 7.40. (a) Calculate the [ H2CO3 ]/[ HCO3 ] ratio. (b) What does the pH become if 15% of the HCO3 ions are converted toH2CO3? (c) What does the pH become if 15% of the H2CO3 molecules converted to HCO3 ions?
A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of solution. What is the pH of the solution after 0.368 mol of HX is added?