Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (M9SO, 7H,O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 73.25 g. What is the mass in grams of the original salt mixture that you must add to 1.000 L of water to make a 0.1000 M solution of Mg2+ ion?

Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (M9SO, 7H,O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 73.25 g. What is the mass in grams of the original salt mixture that you must add to 1.000 L of water to make a 0.1000 M solution of Mg2+ ion?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A 6.57 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

Q: 1. A 5.000 g sample of methanol, CH,OH, was combusted in the presenmce of excess oxygen in a bomb…

A: The given data : The mass of methanol = 5.000 g The mass of water = 4000 g The initial temperature…

Q: The temperature of 82.0 g of water rose from 18.2 °C to 36.2 °C during a chemical reaction. If…

A: In this problem, we are given the mass of water (m), the initial and final temperatures (Ti and Tf),…

Q: A 4.79 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A: Calorimetry is the easiest way to calculate the amount of heat transfer to a substance or from a…

Q: Determine the amount of heat absorbed by a solution in which 485.0 g of NH,NO3is dissolved in water.…

A: enthalpy change given in the question(+25.7kj/mol) is the amount of heat absorbed by the solution…

Q: A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 23.2 mL of 6.45 M hydrochloric…

A: GivenVolume of NaOH solution = 67.0 mL = 0.067 LMolarity of NaOH solution = 2.01 MMoles of NaOH…

Q: I need the third sub part

Q: A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A: Solution : The heat of dissolution is defined as an enthalpy change related to the…

Q: In a calirometer 50.00 mL of 2.50 M NaOH was combined with 50.00 mL of 2.25 M HCl from a solution.…

Q: The solubility of AgCl(s) in water at 25 °C is 1.33 x 10-5 mol/L and its AH of solution is 65.7…

A: AgCl is a sparingly soluble salt. Thus, it is not completely soluble in water but with increase in…

Q: When 1.3 g of KClO3 was added to 151.1 g of water in a calorimeter, the temperature dropped by 0.588…

A: Given, Mass of KClO3= 1.3g Mass of water= 151.1g Temperature dropped(dT)=0.588°C The heat capacity…

Q: When we exercise, we rely on the oxidation of glucose (C6H12O6) to carbon dioxide and water for…

Q: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or…

A: A.) Endothermic reaction is that in which heat is absorbed and temperature fall down. Exothermic…

Q: The change in enthalpy (heat of solution) for ammonium nitrate dissolving in water is 25.7 kJ/mol.…

A: Given, The change in enthalpy (heat of solution) for ammonium nitrate dissolving in water is 25.7…

Q: The change in enthalpy (heat of solution) for ammonium nitrate dissolving in water is 25.7 kJ/mol.…

A: Molar mass of ammonium nitrate =80.043g/mol

Q: A constant pressure (or coffee cup calorimeter) contains 125g of water at a temperature of 24.2°C.…

A: Given , mass of water = 125 ginitial temperature, Ti=24.2°Cmass of KBr added = 10.5 gFinal…

Q: Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (as shown) at 22.4 °C causes the…

Q: A student performs a calorimetry experiment. The student combines 100. g of 0.40 M HC1(aq) with 100.…

A: Heat absorbed by the particular species = mass × heat capacity × temperature change

Q: The enthalpy of dissolution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH,NO3 is…

Q: A chemist placed a 1.195 g sample of fuel in a bomb calorimeter which was immersed into 2.00 L of…

A: The mass of the fuel sample is = 1.195 g The increase in the temperature of the water is = 20.1oC to…

Q: When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee- cup…

A: 1) Since the temperature of the water in coffee-cup calorimeter is decreasing from 22 to 16.9 oC…

Q: A 150.0 mL sample of 0.250 M NaOH is mixed with a 100.0 mL sample of 0.289 M HNO3 in a coffee cup…

Q: Ignition wires heat Thermometer A bomb calorimeter, or a constant volume calorimeter, is a Stirrer…

A: Molar heat of combustion of a substance is defined as the heat liberated during the complete…

Q: 6.00 g of a water soluble salt was dissolved in 75.0mL of water. The initial temperature of the…

Q: You place 50.0 mL of a 0.500 M solution of NaOH in a coffee-cup calorimeter at 25.00°C. You then…

A: Same amount of reactant gives same amount of product. As we can see here.

Q: A 4.77 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

Q: When 15.3 g of sodium nitrate was dissolved in water in a calorimeter, the temperature fell from…

Q: The temperature of 89.3 g of water rose from 17.3 °C to 38.6 °C during a chemical reaction. If…

A: The given values in the problem are:Mass of water (m) = 89.3 gInitial temperature (Ti) = 17.3…

Q: 2 CH3OH) +3 O2(g) → 2 CO2) + 4 H20) + 347 kcal Calculate the amount of heat in kcal & kJ released…

A: Given : The reaction equation is as follows. 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) + 347 kcal Mass…

Q: The compound sodium thiosulfate pentahydrate, Na, S, O3-5H2O, is important commercially to the…

A: The reaction taking place is given as, => S8 (s) + Na2SO3 (aq) + H2O (l) → Na2S2O3·5H2O (s)…

Q: A chemist dissolved an 10.2g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When…

Q: Suppose you had used 4.00 grams of NaOH(s) in Reaction 1. What would have been the number of Joules…

A: The equation given is NaOH (s) → Na+ (aq) + OH- (aq) For the dissociation and dissolution of NaOH…

Q: Need help with #4

A: The balanced reaction taking place is given as, => CuSO4 + 2 KOH → K2SO4 + Cu(OH)2 Given:…

Q: A 8.17 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

Q: In winemaking, microorganisms break down the sugar in grapes into ethanol (grain alcohol) and carbon…

A: The molar mass of ethanol = 46 g 2 moles of ethanol , which weights 92.16 g produces 16.6 kcal of…

Q: When 3.02 g of NH4Cl is dissolved in enough water to make 20.05 mL of solution, the temperature…

A: To find enthalpy change, first find q of reaction by using formula of q. Then divide the calculated…

Q: Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A…

A: Balance chemical equation is defined as which has equal number of atoms or ions in both sides…

Q: What is the enthalpy change in kJ of a chemical reaction that raises the temperature of 250.0 mL of…

A: We have to calculate the enthalpy change

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

Your lab partner accidentally mixed some sodium chloride with your
sample of Epsom salts (M9SO,·7H,O). You want to make a standard
solution of magnesium ion, and this is the only sample of a
magnesium salt you have. To determine the amount of magnesium
salt in the mixture, you heat 100.00 g to drive off the water of
hydration and find that the anhydrous mixture has a mass of 73.25 g.
What is the mass in grams of the original salt mixture that you must
add to 1.000L of water to make a 0.1000 M solution of Mg2+ ion?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Given

Solution

Answer

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

2NO2 (g) ↔ N2O4 (g) 30 mL of NO2 gas is compressed in a syringe to 15 mL. Is this reaction endothermic or exothermic?
For this question, you are trying to determine which beaker will have more heat absorbed and why. You start with two beakers that both contain 50 grams of solution. Beaker 1 contains water (the specific heat capacity for water is approximately 4.2 J/g∘∘C). Beaker 2 contains alcohol (the specific heat capacity is approximately 2.2 J/g∘∘C). Initially, both solutions are at 20∘∘C (about room temperature). Both beakers are then heated to 90∘∘C. Which beaker will have MORE heat absorbed? Explain why. neat handwriteing please and thankk you so muchh
Is dissolving AgNO3 in water an exothermic or endothermic process? What about dissolving MgSO4 in water?
A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.71 °C. Calculate the enthalpy of solution, AH30ln , per mole of salt dissolved. Assume the specific heat of the solution is 4.15 J/(g.C) and the heat capacity of the calorimeter is 5.30 J/°C. Calculate the heat change experienced by the calorimeter contents, qcontents - 9contents = J Calculate the heat change experienced by the calorimeter, qcal - 9cal = J Calculate the heat change produced by the solution process, qsoln - Isoln = J Calculate AHsoln , the enthalpy of solution for one mole of solid in kilojoules per mole. ΔΗon= kJ/mol
A 5.29 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. a)If 3132 J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 5.29 g of salt? b) how many moles of the unknown salt were used in the reaction? c) What was the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
In a coffee-cup calorimeter, 100.0 mL of 1.1 M NaOH and 100.0 mL of 1.1 M HCL are mixed. Both solutions were originally at 24.5°C. After the reaction, the final temperature is 31.9°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCL by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH = kJ/mol
A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 145.0 g/mol145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 ∘C25.00 ∘C to 23.87 ∘C23.87 ∘C . Calculate the enthalpy of solution, Δ?solnΔHsoln , per mole of salt dissolved. Assume the specific heat of the solution is 4.13 J/(g⋅∘C4.13 J/(g⋅∘C ) and the heat capacity of the calorimeter is 3.30 J/ ∘C3.30 J/ ∘C . Calculate the heat change experienced by the calorimeter contents, ?contentsqcontents . ?contents=qcontents= JJ Calculate the heat change experienced by the calorimeter, ?calqcal . ?cal=qcal= JJ Calculate the heat change produced by the solution process, ?solnqsoln . ?soln=qsoln= JJ Calculate Δ?solnΔHsoln ,…
If 0.067 mol of hydrochloric acid (HCl) is mixed with 0.067 mol of sodium hydroxide (NaOH) in a "coffee cup" calorimeter, the temperature of 5.1 g of the resulting solution increases from 25.0 ° C to 34.0 ° C. Given that the energy released is 2.2 × 101 cal when the specific heat of the resulting solution is 1.00 cal/g− ° C, use a conversion factor to convert the energy released to joules (J). Enter your answer in scientific notation. Be sure to answer all parts.
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What is the total mass inside the calorimeter in grams?
Commercial cold packs consist of solid ammonium nitrate and water. NH4NO3 absorbs 25.69 kJ of heat per mole dissolved in water. In a coffee-cup calorimeter, 3.40 g NH4NO3 is dissolved in 100.0 g of water at 21.0 °C. What is the final temperature of the solution? Assume that the solution has a specific heat capacity of 4.18 J/g·C
A 6.57 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. L L L L What is the total mass inside the calorimeter in grams? What is the change in temperature, in °C, inside the calorimeter? Was the dissolution process endothermic or exothermic? What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g. °C. What is the total heat for the dissolution reaction of the 6.57 g of salt? What quantity in moles of the unknown salt were used in the reaction? >
When 1.75 g of CaCl2 dissolves in 125 g of water in a coffee-cup calorimeter, the temperature increases by 2.44°C. What is the heat change per mole of CaCl2 dissolved in water? Assume that all the heat is absorbed by the water (c = 4.18 J/g·°c).