1. How many moles of ions are in the following
solutions: 32.5mg potassium sulfate in water; 1 mol MgBr2 in
C6H6?
2. Given the following reaction and solubility data, how many moles
of total ions are in solution once the reaction is complete
starting with 25g of each reactant in 1L?
Na3PO4 + Ca(NO3)2 --> NaNO3 + Ca3(PO4)2
COMPOUND SOLUBILITY
SODIUM PHOSPHATE 94.6g/100mL
CALCIUM NITRATE 120g/100mL
SODIUM NITRATE 91.2g/100 mL
CALCIUM PHOSPHATE 2mg/100mL
1. Mass of K2SO4 = 32.5 mg = 32.5 *10-3 g = 0.0325 g
Molar mass of K2SO4 = 174.259 g/mol
Moles of K2SO4 = mass/ Molar mass = 0.0325 g / ( 174.259 g/mol) = 1.865 *10-4 mol
Thus, moles of K+ = 2* 1.865 *10-4 mol = 3.73 *10-4 mol
moles of SO42- = 1.865 *10-4 mol
Hence the total moles of ions produced = (1.865 *10-4 mol )+ (3.73 *10-4 mol) = 5.60 *10-4 mol
(b) MgBr2 is a polar but C6H6 is non- polar
SO both are insoluble
Hence, there is no ion
2.
Reaction is:
Na3PO4 + Ca(NO3)2 --> NaNO3 + Ca3(PO4)2
Mass of Na3PO4 = 25 g
Molar mass of Na3PO4 = 163.94 g/mol
Moles of Na3PO4 = 25/ 163.94 = 0.152 mol
Mass of Ca(NO3)2 = 25 g
Molar mass of Ca(NO3)2 = 164.088 g/mol
Moles of Ca(NO3)2 = 25 /164.088 g/mol = 0.152 mol
Thus,Moles of NaNO3 = moles of Ca3(PO4)2 = 0.152 mol
From solubility , Ca3(PO4)2 is insoluble. so, didn;t ionize
Only , NaNO3 will ionize into Na+ and NO3- = 2 ions
hence total moles of ions formed = 2* 0.152 = 0.304 moles
1. How many moles of ions are in the following solutions: 32.5mg potassium sulfate in water;...
If 7.79 grams of calcium nitrate, Ca(NO3)2, react with excess sodium phosphate, Na3PO4, according to 3Ca(NO3)2 + 2Na3PO4 Ca3(PO4)2 +6NaNO3 what is the theoretical yield of sodium nitrate, NaNO3, in grams? (Enter your answe the hundredth place.)
If 3.37 grams of calcium nitrate, Ca(NO3)2, react with excess sodium phosphate, Na3PO4, according to 3Ca(NO3)2 + 2Na3PO4 +Ca3(PO4)2 +6NaNO3 what is the theoretical yield of sodium nitrate, NaNO3, in grams? (Enter your answ the hundredth place.)
1. How many moles of Ca(NO3)2*4H2O are in 50.0 mL of 0.0906 M Ca(NO3)2*4H2O? Report your answer with 3 significant figures. Do not include units. 2. How many moles of Na3PO4*12H2O are in 50.0 mL of 0.0550 M Na3PO4*12H2O? Report your answer with 3 significant figures. Do not include units. 3. If 50.0 mL of 0.0906 M Ca(NO3)2*4H2O are reacted with 50.0 mL of 0.0550 M Na3PO4*12H2O, using the balanced chemical equation from the video, determine which is the limiting...
Balance the reaction below and determine how many grams of nickel(II) phosphate will be formed when sodium phosphate (12.05g) is mixed with nickel(II) nitrate (175 mL, 0.500 M). After the reaction is complete, what is the concentration of the unprecipitated ion (either POX or Ni2+). Na3PO4 + Ni(NO3)2 — Ni3(PO4)2+ + NaNO3
how many moles of calcium ions are there if you completely dissolve 32.6g Ca3(PO4)2 in 1 liter of water?
Write the molar equation and net ionic equation for each reaction. Reaction 1. silver nitrate + sodium chloride AgNO3 Nach 2. silver nitrate + sodium bromide AS Noz doim Narse 3. silver nitrate + potassium iodide A No3 KI 4. silver nitrate + sodium phosphate AS NO3 Naz PO 4 5. barium nitrate + potassium sulfate BaCNO3)2 Krsou 6. lead(II) nitrate + potassium sulfate Tome Pb(NO372 ksoy 7. barium chloride + sodium phosphate Dim Back Na₃PO4 8. calcium nitrate +...
Question 1 According to the following reaction, what mass of silver nitrate would be required to react with 0.500 grams of potassium chloride? AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq) options 2.68 g 0.500 g 85.0 g 170 g 1.14 g Question 2 Consider the reaction: Na2CO3 (aq)+ 2 HCl (aq) --> 2 NaCl (aq) + CO2 (g) + H2O (l) If 43.41 g of sodium carbonate react completely, how many grams of HCl will be...
MOLARITY REVIEW 1.) How many nitrate ions are present in a 25.00mL sample of a 2.50M calcium nitrate solution? 2.) How many mL of a 0.300M lead(II) nitrate solution are needed to react with 50.00mL of a 0.500M potassium chromate solution? (solution stoichiometry problem) 3.) How many mL of a 0.700M Ca(NO3)2 solution are necessary to react with 25.00mL of a 1.000M H2SO4 solution? 4.) 25.66mL of a solution hydroxide solution reacts with 22.55mL of a 0.888M phosphoric acid solution,...
Double Replacement potassium carbonate (aq) + silver nitrate (aq) → potassium nitrate (aq) + silver carbonate (s) K2CO3(aq) + AgNO, (ag) - potassium carbonate (aq) + copper (II) nitrate (aq) potassium nitrate (aq) + copper (II) carbonate (8) K,CO, (aq) + _Cu(NO, ),(aq) potassium carbonate (aq) + aluminum nitrate (aq) + potassium nitrate (aq) + aluminum carbonate (3) K.CO; (aq) + _Al(NO3) (aq) - sodium phosphate (aq) + silver nitrate (aq) sodium nitrate (aq) + silver phosphate (8) Na, PO...
Exp 9 Translating Word Equations into Balanced Chanical Equations A. Combination Reactions Instructor Demonstrations 1. magnesium(s) + oxygen(g) magnesium oxide(s) + 02() 4 Mg(s) 2. sulfur(s) + oxygen(g) 4 sulfur dioxide(g) S(8) + O2(E) B. Decomposition Reactions 1. copper(II) sulfate pentahydrate(s) copper(II) sulfate(s) + water(s) CuSO4.5H20() 2. sodium hydrogen carbonate(s) 4 sodium carbonate(s) + water(g) + carbon dioxide(g) NaHCO3(-) C. Single-Replacement Reactions 1. copper(s) + silver nitrate(aq) + copper(II) nitrate(aq) + silver(s) Cu() + AgNO3(aq) → 2. magnesium(s) + hydrochloric...