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- -6 -5 -4 -3 -2 -1 +1 +2 +3 +4 +5 PbsO.(s) + H*(aq) + 2CI (aq) = Pb(s) + HSO. (aq) + Cl2(g)1. What is the conjugate base of the formic acid HCO,H? 2. You have a 5.43 x 10 M solution of HNO, at 25 °C. Calculate the [OH] of this solution? 3. A solution that has a pH of 4.5 is (acidic, basic, neutral)? 4. A solution has a hydronium ion concentration of 3.2 x 10 M. Calculate the pOH.Adding acid to the buffer, NH3-NH4*, will produce this (net ionic) reaction: H*(aq) +OH(aq)=H₂O(1) H*(aq)+NH4*(aq) NH3(aq)+H₂(g) O H*(aq) + NH4+ (aq)=NH5²+ (aq) O H*(aq)+NH3(aq)=NH4+ (aq)
- Chloride ions are added to the AglAg* half-cell of the cell Ag|Ag*l|Cu²*|Cu to precipitate AgCI (s). The cell voltage is then measured to be +0.072 V at 298 K. If [Cu2+] = 1.0 M in the Cu2+|Cu half cell, what is [Ag*] in the Ag|Ag* half-cell? (First step: You will need to use the data in Table 17-1 to calculate E°cell.) Give your answer to two significant figures. Ecell = E°cell - (0.0257 V/n) In(Q) E'cell = E°ox + E°redChemistry 4+ 3+ 2+ Sn²+ (aq) + 2Fe³+ (aq) →→2Fe²+ (aq) + Sn** (aq) Seleccione una: a. -0.46 Ob. +0.46 C. +1.39 d. +0.617 Half-reaction Cr³+ (aq) + 3e E° (V) -0.74 Fe2+ (aq) + 2e -0.440 Fe3+ (aq) + e Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 Table 20.2 Cr (s) → Fe (s) →cyanate ion in waste solutions from gold mining operations can be destroyed by treatment with hypochlorite ion in basic solution. write a balanced oxidationp-reduction equation for this reaction OCN-(aq) + OCI-(aq) + OH-(aq) --> CO32-(aq) + N2(g) + Cl-(aq) + H2O(l) hint: notice that in the oxidation of half-reaction, OCN- yields to two products
- 5. Balance the following reaction. HCl(aq) + KMn04 (aq) +H2O2 (aq)MnClz (aq) +02 () +KCI (aq) + H20 (1) in an acid solutio a. When a reaction is said to be in an acid solution, what species are most commonly present?I need the equation for Ni2+(aq) plus sodium hydroxide and dimethylglyoximeGiven the following reaction, which occurs in acid solution: CH3CH2OH(l) + Cr2O72-(aq) -> CH3COOH(aq) + Cr3+(aq) Balance this equation using the half equation method.
- Calculate Keq for the reaction Ag+ (aq) + Fe2+ (aq) ⇄ Ag(s) + Fe3+Ag+ + e- → Ag +0.80 VFe3+ + e- → Fe2+ +0.77 VProvide your answer rounded to 2 significant figures.Oxalic acid ionizes in two stages in aqueous solution: H2C2O4(aq) + H2O(€ )2H;0* (aq) + HC2O4 (aq) Kal = 5.9 × 10² HC,O, (aq) + H,O(e)2H;0*(aq) + C20?¯(aq) K22 = 6.4 × 10-5 Calculate the equilibrium concentrations of C¿O²¯, HC,O, H,C,O4, and OH- in a 0.10 M solution of sodium oxalate (Na,C¿O4).2 Pb(NO3)(aq) +SnCl4(aq) --> 2 PbC|2 + Sn(NO3)4
