A surface water is coagulated with a dosage of 30 mg/L ferrous
sulfate and an equivalent dosage of hydrated lime (Ca(OH)2).
2FeSO4*7H2O + 2Ca(OH)2 +
0.5O2 -> 2Fe(OH)3 + 2CaSO4 + 13
H2O
A ) How many pounds of ferrous sulfate are needed per MGD of
water treated.
B) How many pounds/mil of hydrated lime are required assuming, a
purity of 70% CaO?
C) Determine the pounds of Fe(OH)3 sludge are produced per MGD
of water treated.
Q3. When sodium sulfate and barium nitrate react, barium sulfate
and sodium nitrate are formed. What mass of barium sulfate is
obtained when 100.0 mL of 0.105 M sodium sulfate is added to 50.0
mL of 0.0850 M barium nitrate?
A) 0.992 g
B) 2.45 g
C) 2.98 g
D) 3.68 g
E) 1.98 g
Q4. Write the net ionic equation for the reaction between
hypochlorous acid and sodium hydroxide?
Q6. Suppose you have 100.00 ml of a solution...
part 1 You have 2.21 L of water which contains 25 mg/L of PO43–.
What is the total amount of phosphate in the sample? in g -----
part2 The label on a bottle of "organic" liquid fertilizer
concentrate states that it contains 8.40 grams of phosphate per
100.0 mL and that 16.0 fluid ounces should be diluted with water to
make 32.0 gallons of fertilizer to be applied to growing plants.
What version of the dilution equation can be used...
If calcium sulfate and barium sulfate do not form mixed crystals
(i.e. they only form 1:1 species), what is the maximum fraction of
the barium ion that can be precipitated as the sulfate from a
solution that is initially 0.080 M in Ba2+ and 0.100 M in Ca2+,
before the precipitation of calcium sulfate starts? For BaSO4, Ksp
= 1.1 x 10-10, for CaSO4, Ksp = 2.4 x 10-5
What is the concentration of barium ions in a saturated solution
of barium sulfate?
Ksp(BaSO4) = (2.389x10^-8)
(Please explain in detail where numbers are coming from and
write clearly, if hand written) Thank you