A 3.650-g sample containing bromate and bromide was dissolved in sufficient water to give
290.0 mL. After acidification, silver nitrate was introduced to a 25.00-mL aliquot to precipitate
AgBr, which was fil- tered, washed, and then redissolved in an ammoniacal solution of potassium
tetracyanonickelate(II)
A 1.509-g sample of a Pb/Cd alloy was dissolved in acid and diluted to exactly 250.0 mL in
a volumetric flask. A 50.00-mL aliquot of the diluted solution was brought to a pH of 10.0 with a
NH3+?NH3 buffer; the subsequent titration involved both cations and required 28.89 mL of 0.06990 M
EDTA. A second 50.00-mL aliquot was brought to a pH of 10.0 with an HCN/NaCN buffer, which also
served to mask the Cd²+; 11.56 mL of the EDTA solution were needed to titrate the Pb²“. Calculate
the percent Pb and Cd in the sample.
A 50.00-mL aliquot of a solution containing iron(H) and iron(IU) required 10.98 mL of
0.01500 M EDTA when titrated at pH 2.0 and 23.70 mL when titrated at pH 6.0. Express the
concentration of each solute in parts per million.
Zinc reacts with element X to form a compound used as rat poison. In a chemical analysis, it is found that 3.90g zinc combines with 1.24g X to form the compound with empirical formula Zn3X2. Determine the relative atomic mass of element X.
[Relative atomic mass: Zn, 65]
For the following redox reaction: MnO₄⁻ (aq) + Ni (s) → MnO₂ (s) + Ni²⁺ (aq). Show how you would balance the reaction if it were in an acidic solution.
Nickel metal, Ni (s), was left in a solution of aluminum (III) ions (Al³⁺), iron (II) ions (Fe2⁺), and copper (II) ions (Cu²⁺). What reaction is most likely to be spontaneous? Write a balanced redox reaction equation for the reaction.
A galvanic cell must not have :
For the following galvanic cell: Ag(s) | Ag⁺(aq) || Mg²⁺(aq) | Mg(s), which electrode is the anode?
Which of the following reacts spontaneously with Fe²⁺ according to the redox table?
Which of the following is the SOA (strongest oxidizing agent) according to the redox table?