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Basic Chemistry
- (5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) O 0.0958 M O 0.383 M O 0.767 M O 0.192 Marrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*taq) + NO2(g Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu(aq) * e Reduction-Half reation: Balancing 0 & H and charges: H* + NO3 (aq) + e - NO2(g) H20 Balancing electrons lost & gained and balancing the equation: Cus) NO3 (aq) * H* - Cu(aq) NO2(g) H20arrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*2(aq) + NO2(g) + NO29) Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu*2, (aq) e Reduction-Half reation: Balancing O & H and charges: H* + NO3 (aq) e NO2(g) + 1 H20 Balancing electrons lost & gained and balancing the equation: Cu(s) NO3 (aq) + H* - Cu*(aq) NO2(g) H20arrow_forward
- (27) What is the value of the equilibrium constant (Keq) when the following redox reaction takes place at 727°C? Mn (s) + Sn¹+ (aq) → Mn²+ (aq) + Sn²+ (aq) (A) 2.55 x 10¹3 (B) 2.76 x 10¹8 (C) 7.62 x 1036 (D) 5.23 x 10-15 (E) 3.62 x 10-1⁹ The most convenient form of the equation for this one might not be on your note sheet. I suggest using: RT ECELL -In K nF (28) An archaeologist claims that a bone in her collection is from a saber-toothed tiger that is believed to have the carbon-1arrow_forward(7.1b) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. b) Mn*2(aq) + BiO3 (aq) Bi* (aq) + Mn04 (aq) Analysis: Oxidation-Half reation: Balancing atoms & charges: Mn*2(aq) Mn04 (aq) H20 - + H* + e Reduction-Half reation: Balancing atoms and charges: BiO3 (aq) H* + Bi* (aq) e H20 Balancing electrons lost & gained Multiply oxidation-half reaction by e's Multiply reduction-half reaction by es Final balanced equation: Continue nextarrow_forwardConsider the unbalanced reaction below occurring in acidic solution: PbO₂ (s) + (aq) Pb2+ (aq) + 1₂(5) Which of the following reactions is the properly balanced net redox reaction? O PbO₂(s) + 21-(aq) + 4H*(aq) O PbO₂(s) +41-(aq) + 4H*(aq) O PbO₂(s) +1-(aq) + 2H*(aq) - O PbO₂(s) + 21-(aq) - 1 Pb2+ (aq) + 12(s) + 2H₂O() Pb2+ (aq) +212(s) + 2H₂O() Pb2+ (aq) + 1₂(s) + H₂O() Pb2+ (aq) + 1₂(s) + O₂(g)arrow_forward
- (10) * Which reaction is an example of both a precipitation and a neutralization? (A) H3PO4(aq) + 3 KOH(aq) –→ K3PO4(aq) + 3 H2O(1) (B) FeC13(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCI(aq) (C) (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H20(1) (D) H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2 H2O(1) (E) 2 C(s) + 02(g) → 2 CO(g) (11) * All of the statements regarding redox reactions are true except (A) a reducing agent causes another substance to be reduced. (B) halogens usually behave as oxidizing agents because they readily gain electrons. (C) metal ions are produced when pure metals are oxidized. (D) when a substance is oxidized its charge (or oxidation number) decreases. (E) alkali metals often behave as reducing agents because they readily lose electrons. (12) In a typical oxidation-reduction reaction the electrons are transferred (A) from the oxidizing agent to the reducing agent. (B) from what is being oxidized to the substance being reduced. (C) from what is being reduced to the substance being…arrow_forward7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s) Sr2 (aq) 2F (aq) 2arrow_forward8) What is the pH of a solution containing 0.280 M weak base, B', with a K, of 3.9 X 107? (10.51) в (ад) + H-0 (1) ВН (аq) + ОН (ад)arrow_forward
- Which of the following is NOT a redox reaction? CO32-(aq) + HSO4-(aq) ==> HCO3-(aq) + SO42-(aq) 2Al(s) + 12H+(aq) + 3SO42-(aq) ==> 2Al3+(aq) + 3SO2(g) + 6H2O(I) 2H2(g) + O2(g) ==> 2H2O(I) 2NaI(s) + Br2(I) ==> 2NaBr(s) + I2(s)arrow_forwardCalculate the molar concentration HCl when 250 mL of 0.10 M HCl are mixed with 150 mL of 0.10 M NaOH in a beaker. (5) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)arrow_forward(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (nq) - Cro, (aq) Analysis: Balancing under acidic condition first (adding H30 & H") Oxidation-Half reation: Balancing atoms & charges: Cr(OH)x) * H20 - Cro, ug * H' + Reduction-Half reation: Balancing atoms and charges: 10 taq H20 Balancing electrons lost & gained Multiply oxidation-half reaction by Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forward
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