Which of these will make a good buffer? a) H2CO3 and CO3^2- b) H2PO4^- and HPO2^2- c) H2O and...
Question:
Which of these will make a good buffer?
a) {eq}H_2CO_3 {/eq} and {eq}CO_3^{2-} {/eq}
b) {eq}H_2PO_4^- {/eq} and {eq}HPO_2^{2-} {/eq}
c) {eq}H2O {/eq} and {eq}NaOH {/eq}
d) {eq}H_2O {/eq} and {eq}HCl {/eq}
Buffers:
Buffers are solutions that are used to control the pH of the solution. They can do so by preventing drastic changes in the pH of the solution when strong acids and bases are added into the solution. Buffers are composed of acidic and basic components.
Answer and Explanation: 1
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The answer is b) {eq}H_2PO_4^- {/eq} and {eq}HPO_2^{2-} {/eq}.
Buffers can be prepared by mixing a weak acid and conjugate base or a weak base...
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Acid-Base Buffers: Calculating the pH of a Buffered Solution
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Chapter 11 / Lesson 8
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Learn how to calculate the pH of a buffer solution. Discover the purpose of a buffer solution, and work through examples using the buffer solution equation.
Related to this Question
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- Which of the following solutions is a strong base? a. 0.1 M HCl b. 0.1 M HC2H3O2 c. 0.1 M NaOH d. 0.1 M NH3
- Which of the following systems could act as a buffer? A. HCl/Cl^- B. NaOH/OH^- C. HSO_4^-/SO_4^{-2} D. H_3O^+/OH^- E. All of the above
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- Which of the following is a buffer system? A. NaCl and NaNO3 B. HCl and NaOH C. H2CO3 and KHCO3 D. NaCl and NaOH E. HCl and H2O
- Which of the following solutions is a weak acid? a. 0.1 M HCl b. 0.1 M HC2H3O2 c. 0.1 M NaOH d. 0.1 M NH3
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- Which of the following substances would be a poor choice for making conductive solutions? a) HCl, KBr, HNO_3 b) NaOH, KOH, LiOH c) C_6H_12O_6, CH_3OH, CH_3CH_2OH
- Which of the following solutions is a weak base? a. 0.1 M HCl b. 0.1 M HC2H3O2 c. 0.1 M NaOH d. 0.1 M NH3
- Which of these mixtures can serve as a buffer solution? a. CH3NH2 and CH3NH3 + Cl- b. NaOH and NaCl c. HBr and KBr d. CH3CH2COOH and CH3CH2COO + K
- Which of the following pairs of substances would make a good buffer solution? A. HC2H3O2(aq) and NaC2H3O2(aq) B. H2SO4(aq) and LiOH(aq) C. HCl(aq) and KCl(aq) D. HF(aq) and NH3(aq)
- Which of these acids is a component in vinegar? a) H2SO4 b) HCl c) HNO3 d) NaOH e) CH3COOH
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- Which of the following would be an ideal buffer solution? 0.20 M HCN / 0.10 M KCN 0.20 M HCl / 0.10 M KOH 0.20 M CH3CO2H / 0.10 M HCO2H 0.10 HCl / 0.010 M KCl Describe how to prepare 500.0 ml of this buffer with maximum buffering capacity.
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- Will a solution that contains HF and NaOH form a buffer? Explain.
- Which is the stronger acid, HCl or H_2O?
- Which acid is stronger: HCl or HNO3?
- What salt is produced by mixing NaOH and H2CO3?
- Which is the least basic and why? NaOCH3 NaSCH3 NaOH CH3CH2Li
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- Which of the following is the most effective buffer system for a pH value of 6.37? a. H_2CO_3/HCO_3^- (Ka1 for H_2CO_3 is 4.3 \times 10^{-7}) b. HCO_3^-/CO_3^{2-} (Ka2 for H_2CO_3 is 4.8 \times 10^{-11}) c. H_2S/HS^- (Ka1 for H_2S is 8.9 \times 10^{-8})
- What is the [ H 3 O + ] for a buffer solution that is 0.2 M in acid and 0.5 M in the corresponding salt if the weak acid has a K a = 5.8 10 7 ?
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- Which of the following combinations would be the best choice to buffer the pH of a solution at approximately 7? A. NaH_2PO_4 B. H_3PO_4 and NaH_2PO_4 C. NaH_2PO_4 and Na_2HPO_4
- Explain why a buffer can be prepared from a mixture of NH_4 Cl and NaOH but not from NH_3 and NaOH.
- What is the net ionic reaction of HCl (a strong acid) with NaOH (a strong base)? a. H + (aq) + OH^{-}(aq) \rightarrow H_{2}O(l) b. H_{2}O(l) \rightarrow H + (aq) + OH^{-}(aq) c. HCl(aq) + NaOH(aq) \rightarrow NaCl(aq) + H_{2}O(l)
- Which of the following is correctly identified? a. NaOH, weak base b. H2SO4, strong acid c. NH3, strong acid d. H2CO3, strong acid
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- What is the pK_a of a compound used to make a buffer of pH 10.65 using 3 times as much conjugate base than the weak acid?
- Which of the following will result in a buffering solution when equal volumes of each are mixed i) 1.127 M HIO and 0.635 M NaOH ii) 0.805 M HBr and 1.61 M CH3NH2 iii) 0.825 M HClO4 and 1.65 M RbOH a) I and II b) I-III c) None d) III only e) I only
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- Which of the following pairs could be used to make a buffer? a. HF and NaF b. HF and NH3 c. HF and NaNO2 d. HNO3 and NaNO3
- Which mixture is a buffer? a. 0.2 M NH3 and 0.1 M NH4Cl b. 0.2 M NaCl and 0.1 M NaCl c. 0.2 M NH3 and 0.1 M NaCl d. 0.2 M KOH and 0.1 M KNO3
- Which combination of the following would acts as a buffered solution?a. HCl and NaCl b. CH3COOH and KCH3COO c. H2S and NaHS d. H2S and Na2S
- Would HCl and NaOH generate a salt derived from a weak acid and a weak base? Explain.
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- Is an aqueous solution of 0.33 M hydrofluoric acid and 0.29 M sodium fluoride a good buffer system? Explain.
- Which of the following is a weak base? a. NaOH b. HF c. CH3NH2 d. H2C2O4 e. Ba(OH)2
- Which of the following has the greatest buffer capacity? 0.40 M CH_3COONa / 0.20 M CH_3COOH.
- Which of the following pairs of substances can be used to make a buffer system? Choose all that apply. a. H2CO3 and Na2CO3 b. H2C2O4 and Na2C2O4 c. HCl and KCl d. HF and LiF e. NaHC2O4 and Na2C2O4
- Which of the following aqueous solutions are good buffer systems? a. 0.12 M acetic acid + 0.15 M sodium acetate b. 0.33 M hydrofluoric acid + 0.29 M sodium fluoride c. 0.20 M potassium hypochlorite
- Write the acid base neutralization reaction between the buffer and the added HCl.
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- What is the salt formed when HCl reacts with sodium hydroxide?
- How does buffer neutralizes added acid?
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