Calculate the number of milligrams of Ag2CrO4 that would dissolve in 400.0mL of distilled water. Use your average Ksp from the experiment. (Average Ksp is 1.58x10^-11)
Calculate the number of milligrams of Ag2CrO4 that would dissolve in 400.0mL of distilled water. Use...
Using value of 1.1×10−10 for the Ksp, calculate how many milligrams of Ag2CrO4 will dissolve in 13.5 mL of H2O?
what volume of water is needed to completely dissolve 4.0 g of Ag2CrO4 (Ksp = 8.0 x 10^-12, MM = 331.8 g/mol)
How many milligrams of silver bromide would dissolve in 1.0 liter of water?
Calculate the solubility of Ag2CrO4 in water at 25°C. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits. (Ksp=1.12x10^-12) Calculate the solubility of Ag, CrO4 in water at 25 °C. You'll find K data in the ALEKS Data tab. Round your answer to 2 significant digits. Flora x 6 ?
Calculate the molar solubility of Ni3(PO4)2(Ksp= 4.74x 10^-32) and use it to determine how much could you dissolve in 450.0 mL of pure distilled water. What would be the concentrations of the ions in solution at equilibrium?
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. Part A MX ( K sp = 5.30×10−11) Express your answer in moles per liter. Part B Ag2CrO4 (Ksp = 1.12×10−12) Express your answer in moles per liter. Part C Ni(OH)2 (Ksp = 5.48×10−16) Express your answer in moles per liter.
Calculate the solubility of CaSO4 (Ksp = 2.4 x 10^-5) in distilled water and in 0.025 M K2SO4 (include acitvity effects). The ionic diameter for Ca^2+ is 0.6, and the ionic diameter for SO4^2- is 0.4.
It is observed that 7.5 mmol of BaF2 will dissolve in 1.0 L of water. Use these data to calculate the value of Ksp for barium fluoride. Question 19 options: A) 1.7 × 10–6 B) 5.6 × 10–5 C) 2.1 × 10–12 D) 7.5 × 10–3 E) 4.2 × 10–7
4. Calculate how grams of compound X would dissolve in 178 mL of water if it has a solubility of 0.375 g/100 g H2O. (2 pts)
AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about the dissolution of AgCl in water at 298 K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl, by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl-] =...