the concentration of OH ions in solutions
Weak soluble ionic compounds do depend greatly on the solution's ph. Not all compounds depend on the pH though because those that have stronger ionic compounds do not need to depend on the ph.
The final pH of the mixture will depend on how much of the strong acid you add. The initial amount of acid will neutralize the alkaline solution, and if there is enough of the strong acid, the final pH will then become acidic, i.e. pH < 7.
The molarity. The hydrogen ion concentration. If given the Ka just use the Henderson-Hasselbach equation pH=pKa+log(base/acid)
The molarity. The hydrogen ion concentration. If given the Ka just use the Henderson-Hasselbach equation pH=pKa+log(base/acid)
An acidic solution has a pH under 7 and a basic solution has a pH over 7.
Weak soluble ionic compounds do depend greatly on the solution's ph. Not all compounds depend on the pH though because those that have stronger ionic compounds do not need to depend on the ph.
pH is an INTENSIVE property as it does not depend on the amount of material present. The pH of 1 ml of solution x is the same as the pH of 100 ml of solution x.
the H+ concentration and the OH- concentration
Sodium bicarbonate, NaHCO3 is alkaline so the pH will be greater than 7. However, the actual pH will depend on the concentration of the NaHCO3 solution.
Neutral solution: pH =7Acidic solution: pH7.
It will all depend on the amount of solution and the amount of acid that you add. It will move the pH closer to 7. If the amount of solution is rather small, the pH will move further towards the acid side.
A solution with a pH of 7 compared to a solution with a pH of 9 would be more acidic.
Dextrose is a solid so it doesn't really have a pH until it is in solution. Once it is in solution, it would depend on what the solvent was and the concentration of the dextrose. So it could range greatly, but most are kept around 6.4.
The final pH of the mixture will depend on how much of the strong acid you add. The initial amount of acid will neutralize the alkaline solution, and if there is enough of the strong acid, the final pH will then become acidic, i.e. pH < 7.
depends on the molarity, but it is usually pH 5.5.
The molarity. The hydrogen ion concentration. If given the Ka just use the Henderson-Hasselbach equation pH=pKa+log(base/acid)
The molarity. The hydrogen ion concentration. If given the Ka just use the Henderson-Hasselbach equation pH=pKa+log(base/acid)