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Let us assume you have a Hydrochloric acid solution of 0.1 M. The pH is - log10[H+]. So log10[0.1] = -1 easy way to remember this is
103 =1000 log 101000 = 3
102 =100 log 10100 = 2
101 =10 log 1010 = 1
100 =1 log 101 = 0
10-1 =0.1 log 100.1 = -1
10-2 =0.01 log 100.01 = -2
So log10[0.1] = -1 and thus pH is - log10[H] = (minus minus 1) = 1
What else can I help you with?
How do i calculate pH given the acid constant?
For a weak acid, HA...HA ==> H^+ + A^- Ka = [H+][A-]/[HA] Plug these values into the Ka equation. You also must know the [HA] that you start with. Solve for [H+] Take -log [H+] = pH
How can one effectively solve buffer problems?
To effectively solve buffer problems, one should first identify the components of the buffer solution (acid and conjugate base), calculate the initial concentrations, and use the Henderson-Hasselbalch equation to determine the pH. Adjusting the ratio of acid to conjugate base or adding more buffer solution can help maintain a stable pH.
How can you solve problems with soil linked with acidity and alkalies?
To address soil acidity, you can add lime to raise the pH level. For alkaline soil, you can amend it with elemental sulfur to lower the pH. It's important to test the soil first to determine the existing pH level before application.
How can you calculate pka valve if pH is given?
You can calculate the pKa value by using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the acid. Rearranging the equation, you can solve for pKa by taking the antilog of both sides after isolating pKa.
A pH of 10 is how many times as basic as a pH of 7?
1,000 to solve: 10=10-10 while 7= 10-7 divide 10=10-10 by 7= 10-7 which yields the answer of 10-10+7= 103 which is 1,000
How do you derive the isoelectric point equation from Henderson hasselbalch equation?
The isoelectric point (pI) is the pH at which a molecule has no net charge. To find pI from the Henderson-Hasselbalch equation, set the net charge of the molecule equal to zero and solve for pH. This equation is derived by considering the acidic and basic dissociation constants of the molecule to calculate the pH at which the net charge is zero.
What is the pH of a solution with H 2.3 x 10-3?
8.64
What is the formula to determine alcohol acidity?
Let ROH represent the alcoholROH <==> RO^- + H+ Ka = [H+][RO-]/[ROH] Solve for [H+] and take the negative log to get the pH
A 0.20 mol L of both acetic and acid and sodium acetate has a pH of?
The pH of a solution containing 0.20 mol/L of acetic acid and its conjugate base, sodium acetate, depends on the specific concentrations of the acid and its conjugate base, as well as the ionization constant (Ka) of the acid. To calculate the pH, you need to set up an equilibrium expression and solve the equation.
What is the most acidic pH 10 pH 3 pH 2 pH 6 pH 8 pH 12 pH 1 pH 75?
pH 1 is the most acidic, as it is closest to 0 on the pH scale. Lower pH values indicate higher acidity.
What solutions is the weakest acid pH of 2.4 pH of 5.2 pH of 6.4 pH of 8.6 or pH of 10.1?
pH=6,4
How do you calculate concentrations of both acid and base in a buffer solution when only given pH value example pH 7.5?
pH = - log [H+] Substitute and solve for [H+]: 7.5 = - log [H+] = 3.16E-8 That is the concentration of H+ ions. Depending on the acid, you calculate concentration of the acid based on this. Kw (dissociation constant) for water = 10^-14 Kw = [H+]*[OH-] Substitute and solve for the concentration of OH- = 3.16E-7 Depending on the base, you calculate the concentration of the base from this.
