Module 3 Lab Assignment: Solubility & Ksp Solid: AgCl Mass of Solid (g) Molarity of Ag+ 100 g Solid: SrSO4 Mass of Solid (g) Molarity of Sr2+ Molarity of SO4^(2-) 100 g Temperature C 25 °C Write the Ksp expression here: Calculate the Ksp value here (Show work): Temperature °C Volume of 25 °C Write the Ksp expression here: Calculate the Ksp value here (Show work): Volume of Distilled Water (mL) 100 mL Distilled Water (mL) 100 mL Molarity of Cl- 1.33038 x 10^-5 1.33038 x 10^-5 5.83095 x 10^-4 5.83095 x 10^-4

Module 3 Lab Assignment: Solubility & Ksp Solid: AgCl Mass of Solid (g) Molarity of Ag+ 100 g Solid: SrSO4 Mass of Solid (g) Molarity of Sr2+ Molarity of SO4^(2-) 100 g Temperature C 25 °C Write the Ksp expression here: Calculate the Ksp value here (Show work): Temperature °C Volume of 25 °C Write the Ksp expression here: Calculate the Ksp value here (Show work): Volume of Distilled Water (mL) 100 mL Distilled Water (mL) 100 mL Molarity of Cl- 1.33038 x 10^-5 1.33038 x 10^-5 5.83095 x 10^-4 5.83095 x 10^-4

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 90QAP: Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of...

See similar textbooks

Similar questions

Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
The following reaction occurs in pure water: H2O(l)+H2O(l)H3O+(aq)+OH-(aq) which is often abbreviated as H2O(l)H+(aq)+OH-(aq) For this reaction, G = 79.9 kJ/mol at 25C. Calculate the value of G for this reaction at 25C when [OH] = 0.15 M and [H+] = 0.71 M.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.
Non-Commercial Substances Hypothesis: Soluble in Test Bond Molecular Structure ΔΕΝ H2O? Result: H20 Solubility Result: Hexane Substance Classification Solubility Hexane? H2O: pS Sodium Na--Br lonic Bromide 1.9 Hexane: I |--| lodine NP C 0.0 Ammonium N/A lonic Carbonate NH4* O O NH4* Sodium N/A lonic Acetate C--H NP C 0.4 H-C-OH C--O PC H-C-OH Glycerol 1.0 H-C-OH O--H PC 1.4 HI
Provide full complete solution do not round off numbers and show proper labelling and cancellations.
entActivity.do?locator-assignment-take Ikanbewy Tfapies Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80×10 at 698 K: 2HI(g) H2(g) + I½(g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of K, A. Increases B. Decreases C. Remains the same The value of Q. A. Is greater than K. B. Is equal to K C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining 50 hp
give Full detailed and accurate solution solution. The calculation for the last delta S value is 47.62 J/K
b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?.co )= -26.41 kcal/mol, AH?.CH,OH()= -48.08 kcal/mol, AG.co )= -32.8079 kcal/mol, AG.CH,OH(@)= -38.69 kcal/mol, The standard heat capacity of various components is given by. CS = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K |Component b x10 e x105 d x10° a -0.291 CH3OH CO 4.55 2.186 -1.92 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
4. Hot springs and thermal vents have been known to kill visitors on Mammoth Mountain due to suffocation when CO2e) displaces O2 in the atmosphere near the vents. a) (DecExp) Using Gibbs free energy, what is the equilibrium constant, KH for this reaction? b) What is the corrected constant KH = for water at 140°F with an ionic strength of 0.05? (DecExp) c) What would be the partial pressure of CO22) in the nearby atmosphere if {CO2} = 0.3 M for the conditions of part b) above? (DecExp)
-4 The solubility of Co(OH), in water at 25 °C is measured to be 6.4 x 10 Use this information to calculate K,, for L Co(OH),. Round your answer to 2 significant digits.