Reaction is 100% in water because water dissolve both of the Reactants CH3Cl and CH3ONa and thus both Reactants react with each other to give product.
Hexane only dissolve only CH3Cl and not CH3ONa because hexane is nonpolar and CH3ONa is polar.
3. (Solubility and equilibrium) Explain the following changes in equilibrium observedin experiments. The explanatio...
3. (Solubility and equilibrium) Explain the following changes in equilibrium observedin experiments. The explanation must consider all compounds and all of major factors. (5 pts) NaCl CH3CI CH3ONA CH3ОCH3 + in water: nearly 100% yield in hexane: nearly 0 % yield
3. (Solubility and equilibrium) Explain the following changes in equilibrium observed in experiments. The explanation must consider all compounds and all of major factors. (5 pts) CH3CI + CH3ONa - сносн. Naci in water: nearly 100% yield in hexane: nearly 0% yield
3. (Solubility and equilibrium) Explain the following changes in equilibrium observed in experiments The explanation must consider all compounds and all of major factors. (5 pts CH CI + CHONa CHOCHE in water nearly 100% yield in hexane nearly 0 yield 4. Basicity and equilibrium) Carralete the following reaction you must show more
3. Solubility and equilibrium Explain the following changes in equilibrium observed in experiments The explanation must considera compounds and all of major factors. 15 pts) CHCI . CHON CH, OCH NI in water nearly 100% viold in hexane nearly 0% yield 4. Basicity and equilibrium) Complete the following reactions you must show more than one possible mechanisms before you choose the better one with a greatly detailed explanation. Then, explain the equilibrium and the explanation must be done in terms...
3. (4 pts)Consider the dissociation of Iron (II) carbonate (FeCO3: Ksp = 2.1 x 10-11) a. Calculate the molar solubility of FeCO3 in water (HINT - assume y = 1 for all ions in this situation) b. Calculate the concentration equilibrium constant (K'sp) for FeCO3 in 0.001 M NaCi. c. Calculate the molar solubility of FeCO3 in 0.001 M Naci.
Q7. Consider the following equilibrium How will each of the following changes affect the equilibrium yield 1) Increasing Pressure of CO &CO. (g) + 6 H,O(l) -c.H.0. (s) + 6 0(g) ΔΕ1-28 16 kJ of CH O. Explain your reasoning. 2) Increasing temperature ) Removing CO 4) Decreasing the volume of the reaction vessel 5) Removing part of CH O, (s) 6) Adding a catalyst Q7. Consider the following equilibrium How will each of the following changes affect the equilibrium...
Saturated, Unsaturated & Supersaturated Solutions Solution, in which the concentration of solute is that determined by its solubility (at given temperature) is called SATURATED solution. One cannot add more solute to such a solution. We also say that a saturated solution is in equilibrium with pure solute: If we add solid Nacl to an already saturated solution of NaCl, that solid remains in equilibrium with dissolved Naci. Solution containing less solute than would be in the saturated solution, is UNSATURATED...
CH2CN-5 3. (Solubility). Explain why the following observation takes place about the Nicotine. (5 pts) Solubility in water increases when pH is acidic.
B. Solubility Equilibrium; Finding a Value for Ksp 2. Explain why PbCl 2 did not precipitate immediately on addition of HCl. What conditions must be met by [Pb2 + ] and [Cl- ] if PbCl 2 is to form? 3. Explain your observations in Steps 3 (The amount of precipitate begins to decrease as it dissolves in the hot water.) and 4 (The precipitate reappears, forming after the test tube was put in ice water.) of the procedure. In which...
Consider the graph showing solubility curves of various ionic compounds. Determine the molarity of a saturated KCl solution at 80 degrees C. Molar mass of KCl is 74.55 g/mol and density of water is 1.00 g/mL 150 KI 140 130 120 110 NaNO3 100 KNO3 90 Grams of solute per 100 g H20 80 70 NH37 60 NHACI 50 -KCI 40 Naci 30 20 KCIÓ: 10 Cez(SO4)3 0 0 10 20 30 40 50 60 70 80 90 100 Temperature...