Write an equation showing why the crude aspirin dissolves in the saturated NaHCO_3 solution.
Why do you add saturated NaHCO3 to your crude aspirin? Why do you later add 3M HCl?
plz help asap 5. Write balanced reaction equations for the reactions involved (a) when aspirin dissolves in aqueous NaHCO3, and (b) when aspirin is pre- cipitated from a sodium acetylsalicylate solution by HCI. Assuming that both reactions are spontaneous under standard conditions, label the stronger acid, stronger base, weaker acid, and weaker base in each equation.
1. Write a chemical equation showing why a sodium carbonate solution is basic. Calculate the pH of a 0.10 M sodium carbonate solution, Na2CO3 (aq).
In the process of the purification of cyclohexene, we used a saturated NaCl solution to wash the crude product instead of the same volume of pure water. Explain why.
Write the reaction equation showing the two starting materials with the sulfuric acid catalyst reacting to give the aspirin product along with acetic acid? Acetic acid is an additional product of this reaction. How is it removed from the aspirin? Why were both ethanol and water used to recrystallize the aspirin?
Write out the balanced chemical equation showing how the sparingly soluble compound gallium hydroxide, Ga(OH)3, dissociates/dissolves in water. Write out the Ksp expression for this equilibrium. Calculate the molar solubility of Ga(OH)3, Ksp = 7.28 x 10-36.
1. Write the acid dissociation reaction equation for Na2H2PO4. 2. Write a reaction equation showing how the buffer solution maintains pH ~ 8.0 upon addition of acid. 3. Write a reaction equation showing how the buffer solution maintains pH ~ 8.0 upon addition of a base. Buffer solution: Acid= Na2H2PO4 base Na2HPO4 4. Would you expect this buffer to be better at resisting a change in pH upon addition of acid, or upon addition of base? Why?
For AgC2H3O2 salt, write a balanced equation showing the solubility equilibrium, write the solubility product expression, and determine the mass that dissolves in 375 mL of water at 25 °C. (for AgC2H3O2, Ksp = 1.94*10-3 )
CaSO4 dissolves into 32.0 °C water. That resultant solution is saturated when you have 0.209 grams of CaSO4 per 100.0 mls of solution. Under these conditions, what is the Ksp of CaSO4? 1.54x102 1.82x10-5 4.37x102 2.36x104 6.02x10-3
Which of the following statements is TRUE of a saturated solution? The solution is completely homogeneous. None of the other statements are true. The concentration of the reactants and products are equal. If additional solute is added to the solution, it readily dissolves. The rate at which solute dissolves is equal to the rate at which the solid forms.