Definition to use for the log (logarithm):
the logarithm of a number (n) to a given base (b) is the exponent (e) to which the base must be raised in order to produce that number.
(Raising to the power is the inverse of taking the logarithm.)
logb(n) = e or be = n
For example, the logarithm of 1000 to base 10 is 3 ( log10(1000) = 3),
because 10 to the power of 3 is 1000: 103 = 1000.
-log10[H+] is (by definition) used to calculate the pH of a dilute solution in which [H+] = concentration of H+ (or H3O+) in mol/L.
pH = -log10[H+] or [H+] = 10-pH
The solution to this problem is simple if you just work backwards. pH= -log10[H+] You already know what your pH is, so write your equation like this: 4.3= -log10[H+] An understanding of basic logarithm properties lets you know that you can rewrite the equation like this: 10-4.3= [H+] 5.0 *10-5 = [H+]
35
(t+h)(x+2)
A=9 h=1 9+9+1=19
The problem is "h+35=15".Subtracy 35 from each side, so h=-20.
pH means -log10(H+concentration) so pH of a H+ concentration 3.6x10-9 is: pH = -log10(3.6x10-9) ≈ 8.4
pH = -log10[H+] = -log10(0.001 mol/L )= -log10(10-3)= 3
pH s calculated as the negative log10 of the hydrogen ion concentration. So log10 of 0.000724 = -3.14 so pH= 3.14
The little 'p' means -log10 (that's the negative log to base 10). Thus pH means -log10(Hydrogen ion concentration) → pH of the solution = -log10(7.0 x 10-2) ≈ 1.15
1.70
The pH is the co-logarithm of the activity of the dissolved ions H+ in a solution. The formula is (a is the activity):pH = - log10 aH
The concentration of H+ [H+] = 0.01 m/l by definition pH = -(log10 (0.01)) therefore pH = 2
pH = -log10[H+], where [H+] is the hydrogen ion concentration. So, in this case, pH = -log10[1], yielding pH = 0.
The little 'p' means -log10 (that's the negative log to base 10). Thus pH means -log10(Hydrogen ion concentration) → pH of the solution = -log10(7.0 x 10-2) ≈ 1.15
pH = -log10[H+][H+] = 10-pH[H+] = 10-3.45[H+] = 3.548 x 10-4 (this is the amount of mols of H+ per L)
pH + pOH = 14 pH is a measure of the hydrogen ion concentration, [H+] pOH is a measure of the hydroxide ion concentration, [OH-] pH = -log10[H+] pOH = -log10[OH-]
pH = -log10 [H+] So 0.001M = -log10 [H+] = 3 10 times higher concentration = 0.01M so -log10 [H+] = 2 The relationship is thus for every 1 unit of pH reduction there is a tenfold increase in concentration.