Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction LiNO3
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Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction LiNO3
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- Use Le Chátelier's principle to explain what happens to the equilibrium H2O(l)H+(aq)+OH(aq) when a few drops of HCl are added to pure water.Please don't provide handwritten solution ...A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Construct an ICE table for the ionization equation described below.. Use the given information to determine the concentration at equilibrium for all reactants and products.. Initial () Change () Equilibrium () 0.050 + x 0.050 + 2x A (aq) 0 0.050- x A (aq) + H₂O(1) HA(aq) + OH(aq) 0.050 - 2x + 0.050 0.100 + x 0.100 + 2x 0.100 0.100 - x H₂O(l) 0.100 - 2x -X (0.050 + x)² = +x (0.050- x)² +2x HA(aq) (0.100 + x)² RESET -2x (0.100 - x)² + OH (aq)
- Please don't provide handwritten solution ....Please don't provide handwritten solution ....a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…
- a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…Please don't provide handwritten solution ....Some NH4Cl dissolves in water and is under equilibrium. What is the effect to pump NH3 (g) into the above NH4Cl solution? The process will not change the solution volume. (Choose one option only.) Options: a. The amount of NH4+ will decrease, and the solution pH will increase. b. The amount of NH4+ will decrease, and the solution pH will decrease. c. The amount of NH4+ will increase, and the solution pH will decrease. d. The amount of NH4+ will increase, and the solution pH will increase. e. Adding NH3 into the solution has no effect on the solution pH.
- The equilibrium constant expression for the second ionization step of phosphoric acid (Ka2) will contain __________ in the numerator (top). Adding heat to an endothermic reaction will _________. decrease the amount of product increase the amount of reactants shift the equilibrium to the left all of the above none of the aboveIdentifying the major species in weak acid or weak base... The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCN is a weak acid. acids: 1.9 mol of KOH is added to 1.0 L of a 1.0M HCN bases: solution. O other: 0.095 mol of HNO, is added O acids: to 1.0 L of a solution that is bases: 1.4M in both HCN and KCN. O other: O O D O O DA few small drops of water are left in a burette that is used to titrate a base into an acid solution to determine the concentration of the acid. Will this small amount of water have any effect on the determined value for the concentration of the acid? If so, how is it affected? a. Those extra few drops of acid will cause the calculation for the concentration of the base to be too low. This is because it will seem that it took more acid to neutralize the base than it really did and so it will appear that the base is of stronger concentration than it really was. b. Those extra few drops of acid will cause the calculation for the concentration of the base to be too low. This is because it will seem that it took less acid to neutralize the base than it really did and so it will appear that the base is of stronger concentration than it really was. c. Those extra few drops of acid will cause the calculation for the concentration of the base to be too high. This is because it will seem that…