1.  A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a)  Write the titration reaction.  (b)  Calculate the %FeO (M.M. = 71.85) in the sample.   2.  A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a)  Write the titration reaction.  (b)  Calculate the molarity of the titrant solution.    Box the final answer.

3. Calculate the [Ag"] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough water to make 1.00 L of solution. Kf[Ag(CN)2] = 1.0 x 102 1-

Explain why copper(II) and iodide ions do not co-exist in acidic solution but do co-exist in the presence of ammonia. I want solution ASAP

Define: (a) ore; (b) mineral; (c) gangue; (d) brine.

A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate.  a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?

A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron   ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.

A solution is prepared by mixing the two solutions together. The first solution is 150.0 mL and contains 30.78 mM Ti3+, 29.40 mM Ce3+, and 8.75 mM HCI. The second solution is 200.0 mL and contains 40.23 mM EDTA and 11.48 mM piperidine. Determine the concentration of free (non-complexed) metals when the two solutions are mixed.

A 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3.  - What is the equation for I2 * starch deep blue color disappearance?

What is the reaction resulting from the addition of SnCl2(aq) to a solution containing Bi3+ in a basic solution?