5310 4 mol L Submit My Answers Give Up Correct Cyanide Poisoning When species

# 5310 4 mol l submit my answers give up correct

This preview shows page 13 - 16 out of 19 pages.

5.3×10 −4 mol/ L Submit My Answers Give Up Correct ± Cyanide Poisoning When species combine to produce a coordination complex , the equilibrium constant for the reaction is called is the formation constant , K f . For example, the iron(II) ion, Fe 2+ , can combine with the cyanide ion, CN , to form the complex [Fe(CN) 6 ] 4− according to the equation Fe 2+ (aq)+6CN (aq)⇌[Fe(CN) 6 ] 4− (aq) where K f =4.21×10 45 . This reaction is what makes cyanide so toxic to human beings and other animals. The cyanide ion binds to the iron that red blood cells use to carry oxygen around the body, thus interfering with the blood's ability to deliver oxygen to the tissues. It is this toxicity that has made the use of cyanide in gold mining controversial. Most states now ban the use of cyanide in leaching gold out of low-grade ore. Part A The average human body contains 5.00 L of blood with a Fe 2+ concentration of 1.70×10 −5 M . If a person ingests 6.00 mL of 25.0 m M NaCN , what percentage of iron(II) in the blood would be sequestered by the cyanide ion? Express the percentage numerically. 29.4 % Fe 2 + Submit Hints My Answers Give Up Review Part Correct Chapter 17 Reading Question 8 Part A Solid zinc hydroxide, Zn(OH) 2 , is equilibrated with a solution that is buffered at pH 7.82. If the K sp for Zn(OH) 2 at 25°C is 3.0 × 10 –16 , calculate the molar solubility of Zn(OH) 2 in this buffered solution. Solid zinc hydroxide, Zn(OH) 2 , is equilibrated with a solution that is buffered at pH 7.82. If the K sp for Zn(OH) 2 at 25°C is 3.0 × 10 –16 , calculate the molar solubility of Zn(OH) 2 in this buffered solution. 1.7 × 10 –4 M 4.2 × 10 –6 M 4.5 × 10 10 M 6.9 × 10 –4 M Chapter 17 Reading Question 9 Part A Given that the K sp for CaF 2 at 25°C is 3.9 × 10 –11 , will a precipitate form when 0.10 L of 2.3 × 10 4 M CaCl 2 is added to 0.50 L of 5.0 × 10 –3 M NaF? Assume volumes are additive. Given that the K sp for CaF 2 at 25°C is 3.9 × 10 –11 , will a precipitate form when 0.10 L of 2.3 × 10 4 M CaCl 2 is added to 0.50 L of 5.0 × 10 –3 M NaF? Assume volumes are additive. No, because Q = 6.6 × 10 –10 and therefore Q > K sp . Yes, because Q = 6.6 × 10 –10 and therefore Q > K sp . Yes, because Q = 5.8 × 10 –9 and therefore Q > K sp . Yes, because Q = 1.6 × 10 –7 and therefore Q > K sp . Submit Hints My Answers Give Up Review Part Correct Problem 17.68 Part A Using the value of K sp =6×10 −51 for Ag 2 S , K a 1 =9.5×10 −8 and K a 2 =1×10 −19 for H 2 S , and K f =1.1×10 5 for AgCl −2 , calculate the equilibrium constant for the following reaction: Ag 2 S(s)+4Cl (aq)+2H + (aq)⇌2AgCl −2 (aq)+H 2 S(aq) Express your answer using one significant figure. K eq = 7.64⋅10 −15 Submit My Answers Give Up Correct Problem 17.69 Part A Will Ca(OH) 2 precipitate from solution if the pH of a 6.0×10 −2 M solution of CaCl 2 is adjusted to 8.0? Will precipitate from solution if the of a 6.0×10 −2 solution of is adjusted to 8.0?  #### You've reached the end of your free preview.

Want to read all 19 pages?

• • • 