Determine the PH of a 0.232M mg (OH)2 solution at 25 degree Celsius.
Determine the PH of a 0.232M mg (OH)2 solution at 25 degree Celsius.
The solubility of magnesium hydroxide, Mg(OH)2, is 9.57X10^-3g of Mg(OH)2 per 1000g of saturated Mg(OH)2 solution of 25 degrees Celsius. (i) Express this solubility in mol of Mg(OH)2 per litre of Mg(OH)2 solution. (ii) What is the concentration of each of the component ions in mol L-1 in a saturated solution of Mg(OH)2? (Assume that 1mL of solution has a mass of exactly 1g at 25 degrees Celsius).
Ba(OH)2 was dissolved in pure water at 5 degree celsius until a saturated solution was obtained. the pH of this solution was found to be 12.25 a) what is the solubility of Ba(OH)2 in pure water at this temperature? answer in mol/L b) what is the Ksp of the Ba(OH)2 at this temperature?
(a) Determine the equilibrium constant of Mg(OH)2(s) dissolution at 25 oC. (b) For a solution containing 10-3 M dissolved Mg, at what pH will Mg(OH)2(s) precipitate?
Mg(OH)2 has a Ksp=5.61x10-12. Determine the pH of a saturated solution of Mg(OH)2. (Magnesium hydroxide is a solid.) (10 points)
Calculate [OH-], pH and pOH of a 0.175M KHCO3 solution at 25 degrees celsius *WRITE IN PRINT (LEGIBLY)*
Question 3 The solubility of Mg(OH)2: (58.3 g/mol) is 9.63 mg Mg(OH)2/100.0 mL solution at 25 °C. What is the poH of Mg(OH)2 at this temperature?Question 4 What is the pH of a 0.7 mol/L benzoic acid (C6H5COOH, Ka =6.6x10-5) solution?
Determine the PH for a 0.267 M NaCH3H5O3 solution at 25 degrees Celsius, the Ka for HO3H5CH3 is 1.38x10-4
6) a. calculate pH at 25 degree that is 0.0075 HCLO 4. Determine the pH of a 6.75 X 10-3M Al(OH)3 (5) $5. Calculate the [OH^) in a solution at 25°C in which the pH is 9.03. (5) 6. The Ka for hypochlorous acid (HCIO) is 3.5 x 10-8. (a) Calculate the pH at 25°C that is HCIO. (b) Determine the percent ionization. (10)
Determine the [ OH − ] , pH, and pOH of a solution with a [ H + ] of 8.0 × 10 − 9 M at 25 °C. [ OH − ] = M pH = pOH = Determine the [ H + ] , pH, and pOH of a solution with an [ OH − ] of 0.0047 M at 25 °C. [ H + ] = M pH = pOH = Determine the [ H + ]...
Assuming complete dissociation, what is the pH of a 4.47 mg/L4.47 mg/L Ba(OH)2Ba(OH)2 solution? pH=