When 200.0 ml of 0.270 M Mgcl2 solution reacts with with 300.0 ml of 0.160 M...
When 200.0 ml of 0.270 M Mgcl2 solution reacts with with 300.0 ml of 0.160 M K3Po4 solution a precipitate forms.
A) Determine the molarity of the chloride ion after the reaction has occured.
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When 200.0 ml of 0.270 M Mgcl2 solution reacts with with 300.0
ml of 0.160 M...
A solution of 100.0 mL of 0.200 M KOH is mixed with solution of 200.0 mL...
A solution of 100.0 mL of 0.200 M KOH is mixed with solution of 200.0 mL of 0.150 M NiSO_4. (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?
8. Predict whether or not a precipitate will form when 300.0 mL of 0.100 M CuCl2...
8. Predict whether or not a precipitate will form when 300.0 mL of 0.100 M CuCl2 and 200.0 mL of 0.200 MK2CO3 are mixed. First, determine the formula of the precipitate, and look up its sp.
200.0 mL of a solution of 2.000M MgCl2 was mixed with equal amount of 2.000M Na2CO3and...
200.0 mL of a solution of 2.000M MgCl2 was mixed with equal amount of 2.000M Na2CO3and MgCO3 precipitate was collected (MgCO3 Ksp = 1.580x10?8). How much (how many grams) of the precipitate was collected? What is the final concentration of the [Mg] in the solution? Steps would be appreciated!
Enter your answer in the provided box. If 27.9 mL of silver nitrate solution reacts with...
Enter your answer in the provided box. If 27.9 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.455 g of precipitate, what is the molarity of silver ion in the original solution? M
If 28.6 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.839...
If 28.6 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.839 g of precipitate, what is the molarity of silver ion in the original solution?
If 35.4 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.538...
If 35.4 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.538 g of precipitate, what is the molarity of silver ion in the original solution?
1) For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.5 mL of 0.070 M...
1) For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.5 mL of 0.070 M lead nitrate is added to 19 mL of 0.018 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms. 2) Sodium phosphate is added to a solution that contains 0.0041 M aluminum nitrate and 0.028 M calcium chloride. The concentration of the first ion to...
Sodium phosphate is added to a solution that contains 0.0094 M aluminum nitrate and 0.025 M...
Sodium phosphate is added to a solution that contains 0.0094 M aluminum nitrate and 0.025 M calcium chloride. The concentration of the first ion to precipitate (either Al^3+ or Ca^2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate? Sulfur dioxide reacts with chlorine at 227 degree C: SO_2(g) +Cl_2(g) SO_2Cl_2(g) K_p for this reaction is 5.1 times 10^-2 atm-1. Initially, 1.00 g each of SO_2 and Cl_2 are placed...
Suppose 60.8 mL of a 0.136 M solution of Na2SO4 reacts with 161 mL of a...
Suppose 60.8 mL of a 0.136 M solution of Na2SO4 reacts with 161 mL of a 0.238 M solution of MgCl2 to produce MgSO4 and NaCl as shown in the balanced reaction.Na2SO4(aq)+MgCl2(aq)⟶MgSO4(s)+2NaCl(aq) Determine the limiting reactant for the given reaction. MgSO4 Na2SO4***** NaCl MgCl2 Calculate the mass of MgSO4 that can be produced in the given reaction. mass of MgSO4: g Only 0.430 g of MgSO4 are isolated after carrying out the reaction. Calculate the percent yield of MgSO4. percent...
3. 300.0 mL of a 2.500 M solution X was mixed with 300.0 mL of a...
3. 300.0 mL of a 2.500 M solution X was mixed with 300.0 mL of a 2.500 M solution Y in a calorimeter. Both of the solutions were at the same temperature initially. Determine the heat of neutralization (kJ/mole) if the temperature goes from 12.0 °C to 29.0 °C. Assume a molar ratio of 1:1. The specific heat of the solution is 4.281 J/g °C. The density of the mixture is 1.050 g/mL. 4. Sketch a crude time-temperature graph for...
A solution of 100.0 mL of 0.200 M KOH is mixed with solution of 200.0 mL of 0.150 M NiSO_4. (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?
8. Predict whether or not a precipitate will form when 300.0 mL of 0.100 M CuCl2 and 200.0 mL of 0.200 MK2CO3 are mixed. First, determine the formula of the precipitate, and look up its sp.
Enter your answer in the provided box. If 27.9 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.455 g of precipitate, what is the molarity of silver ion in the original solution? M
Sodium phosphate is added to a solution that contains 0.0094 M aluminum nitrate and 0.025 M calcium chloride. The concentration of the first ion to precipitate (either Al^3+ or Ca^2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate? Sulfur dioxide reacts with chlorine at 227 degree C: SO_2(g) +Cl_2(g) SO_2Cl_2(g) K_p for this reaction is 5.1 times 10^-2 atm-1. Initially, 1.00 g each of SO_2 and Cl_2 are placed...
3. 300.0 mL of a 2.500 M solution X was mixed with 300.0 mL of a 2.500 M solution Y in a calorimeter. Both of the solutions were at the same temperature initially. Determine the heat of neutralization (kJ/mole) if the temperature goes from 12.0 °C to 29.0 °C. Assume a molar ratio of 1:1. The specific heat of the solution is 4.281 J/g °C. The density of the mixture is 1.050 g/mL. 4. Sketch a crude time-temperature graph for...
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