This is at the 'neutral' point, when pH is exactly 7.0 (at room temperature).
This is NOT necessarely the same pH as at equivalence point, the latter can be (somewhat) higher or lower than 7, depending on the substance to be titrated, in acidimetric titrations that is.
(Some oxidimetric or other kind of volumetric titrations the pH can be very different and not changing anyhow).
Adding NaOH will increase the pH of water, because NaOH is a base. At 25°C: pH < 7 is an acidic solution pH = 7 is a neutral solution pH > 7 is a basic solution
the concentration of the titrant and the concentration of the titrate.
The two would partially neutralize each other. The "equal amount" part is meaningless in this case, because we don't know the concentrations. If you meant equal molar amounts of calcium hydroxide and ethanoic acid, you'd wind up with a very slightly basic solution because it takes two moles of ethanoic acid to completely react with calcium hydroxide.
The equivalence point represents a region where the amount of acid to base (or base to acid) concentration is equal. Before the equivalence point there is a greater amount of acid (or base, depending on the titration). After the titration there is a greater amount of base (or acid). This reverse in dominance results in a dramatic change in pH.
salt ions and water and an equal amount of hydrogen and hydroxide ions.
The pH of a solution is related directly to its concentrations of hydronium ions(H3O^+) and hydroxide ions(OH-). Acidic solutions have more hydronium ions than hydroxide ions. Neutral solutions have equal numbers of the 2 ions. Basic solutions have more hydroxide ions than hydronium ions.
No. pH is the negative logarithm of the concentration of the hydronium ion. Equal numbers of hydronium ions and hydroxyl ions occurrs only when a solution is neutral.
The product of hydronium and hydroxide is a constant Kw equal to 1.00*10-14 at 25°C. Therefore, as one increases, the other decreases.
The concentrations of hydronium and hydroxide ions are equal
In an acidic solution, the relative concentration of hydronium ions will always be higher than hydroxide ions. This means that the relatively concentration of hydroxide ions will always be lower than hydronium ions in an acidic solution. The reason for this is that in a neutral solution, the concentration of both hydronium ions and hydroxides ions are equal (both are 10-7). By making the concentration of hydronium ions greater than the concentration of hydroxide ions, the solution becomes acidic.
At pH 7, the concentration of hydroxide and hydrogen (hydronium) ions is equal; both concentrations are equal to 10-7 mol/L.
The hydroxide ion concentration equals the hydronium ion concentration at a (neutral) pH of 7
The concentrations of hydronium and hydroxide ions are equal
There are nearly equal amounts of a conjugate acid-base pair.
A neutral solution has an equal number or concentration of hydrogen and hydroxide ions. A neutral solution is one that has a pH of 7.0. Pure water is a neutral solution.
Completely pure water contains only the ions H+ and OH-.The first answerer had it right for the most part (Hydrogen ions do not exist by themselves in water, but rather as Hydronium ions, or H3O+)Water goes through the reversible process of self-ionization:2 H2O H3O+ + OH-This is why water has a neutral pH; water has equal amounts of Hydroxide and Hydronium ions, unless an acid or base is added to shift the equilibrium.
The concentration of hydronium (or hydrogen) ions in solution is found by raising to to the negative pH. In this case, we know that the pH is 7 because it is neutral, so we would say...[H3O+] = 10-pH[H3O+] = 10-7[H3O+] = 1.0 x 10-7 mol/LNeutral solutions have equal concentrations of H3O+ and OH-, so the hydroxide concentration is the same as the hydronium concentration: 1.0 x 10-7 mol/L.Hope this helps:)