Calculate the number of milliliters (mL) of ammonia whose density is 0.99 g/mL, 2.3% by weight NH3 which will be required to precipitate the iron as Fe(OH)3 in a 0.74 g sample that contains 22% FeO.

Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = M

30.0 mL of 0.322 M potassium iodide are combined with 20.0 mL of 0.530 M lead (II) nitrate. How many grams of lead (II) iodide will precipitate? Pbla 2KNO) + 2Ka Pb(NO,) O a 2.23 g 4.90 g 8.90 g 4.45 g

Give detailed Solution with explanation needed

Fill in the missing words With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the form of Zn(OH)2 with the addition of 6.00 mL of NaOH, the number of moles of Zn2+ in this 10 mL brass stock solution is mmol. Therefore, there are mmol of Zn2+ in the entire 100-mL brass stock solution, which is g/mol). mg of Zn2+ (FW = 65

6. The K, for the salt FeCO, is 3.07 x 10. A student mixes 500. mL of 8.2 x 10 M Fe(NO,), with 500. mL of 8.2 x 10 M Na,CO,. Calculate the molar concentrations of Fe²"c) and CO;²aq) in the 1.00 L of solution. a. b. Does a precipitate occur when the solutions are mixed, or does the solution stay clear? Explain

What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?

7.  The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq)                      (Z) 25.0 mL of 1.0 M CH3COOH(aq)   Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True

Which anion or anions are not present in a solutionthat forms no precipitate upon addition of BaCl2 (aq)?

A 2.45 g mixture of BaCl2 and Ba(NO3)2 is dissolved in water.  Excess AgNO3 is added and all of the dissolved chloride ion is precipitated. The resulting precipitate weighs 0.845 g.  Use the following Molar Masses (in g mol−−1) as required: Ba: 137.3 Cl:  35.45 Ag: 107.9 N: 14.01 O: 16.00   What is the mass of Ba(NO3)2 in the original mixture?  Enter a mass accurate to three significant figures.  g