A geochemist in the field takes a 46.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X. He notes the temperature of the pool, 30.° C, and caps the sample carefully. Back in the lab, the geochemist filters the sample and then evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 10.6 g. yes Using only the information above, can you calculate the solubility of X in water at 30.° C ? no If you said yes, calculate it. Be sure your answer has a unit symbol and 3 significant digits.

A geochemist in the field takes a 46.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X. He notes the temperature of the pool, 30.° C, and caps the sample carefully. Back in the lab, the geochemist filters the sample and then evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 10.6 g. yes Using only the information above, can you calculate the solubility of X in water at 30.° C ? no If you said yes, calculate it. Be sure your answer has a unit symbol and 3 significant digits.

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

Similar questions

An enthalpy of solution discusses the enthalpy change of dissolving an ionic compound in water. 8.31 grams of NaOH is added to 152.5 mL of H2O at 298 K. What is the final temperature of this solution after the salt dissolves if the enthalpy of solution for NaOH is -44.5 kJ/mol? The heat capacity of water is 4.184 J/ (g K) and the density of water is 1.00 g/mL.
5.21 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
3.56 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
What is qH2O?
8.96 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or endothermic?
Two 1-L beakers, A and B, each containing a different aqueous solution of fructose (a nonvolatile sugar with MW = 180.16 g/mol) are placed together in a box, which is then sealed. The temperature remains constant at 20 °C. Initially, there is 220 mL of solution in A and 650 mL of solution in B. As the solutions stand in the sealed box, their volumes change slowly for a while. When they stop changing, beaker A contains 430 mL and beaker B contains 440 mL. It is then determined that the solution in A is 1.74 M in fructose and has a density of 1.12 g mL-¹. (a) What is the molar concentration of fructose in the solution in beaker B at the end? M (b) Calculate the concentration of fructose in the solution in A at the start. M (c) Calculate the concentration of the fructose in the solution in B at the start. M (d) The vapor pressure of pure water at 20 °C is 17.5 torr. What is the pressure of water vapor in the box at the end, after the volumes have stopped changing? torr
Cold packs (like the kind used by athletes to treat sprains and other minor injuries) rely on the fact that the enthalpy of dissolution of ammonium nitrate is positive. Is this an exothermic or endothermic reaction? Exothermic Endothermic Neither because this is a closed system and therefore no heat is lost.
When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC. After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 107.87 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures. What is the heat transferred by this reaction, in Joules?