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It depends on what compound is dissolved in what solvent.
Presuming a strong monoprotic acid (eg. HCl) in water the pH is equal to -log[H+] = -log(6.8*10^-3) = 3-log6.8 = (3-0.8) = 2.2
Presuming a strong monoprotic base (eg. NaOH) in water the pH is equal to 14 - pOH = 14 - (-log[OH-]) = 14+log(OH-) = 14 + log(6.8*10^-3) = 14 + (-3 + log6.8) = 14 + (-3+0.8) = 14 - 2.2 = 11.8
Fot pH calculation of weak acids and bases you'll need more complex formula and approximations.
What else can I help you with?
What is the pH of a solution that has a concentration of hydrochloric acid equal to 0.001 M?
Remembwer pH is = the negative logarithm to base ten, of the hydrogen ion concentration . So with a concentration of 0.001 M The hydrogen ion concentration is 0.001 = 10^(-3) ph = -log(10)[H^+] pH = -log(10)10^-3 pH = -(-3) log(10)10 ( Remember log(10)10 = 1 ) pH = -(-3)(1) = --3 = 3 pH = 3
What is the pH of a 1.6 10-3 M HNO3 solution?
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
What is the pH of a solution with H plus 2.3 10 -3?
5.0 x 10-3 pH = - log [H3O+] [H3O+] = 1 x 10^-pH pH = 2.3 [H3O+] = 1 x 10^(-2.3) = 5 x 10^(-3) M
What is the pH of 1x10-3 H?
- log(1 X 10 -3 M H +) = 3 pH =====
What is the pH for 1.0 times 10 -3 m hcl?
The pH of a 1.0 x 10^-3 M HCl solution is 3.00. This is because HCl is a strong acid that dissociates completely in water to form H+ ions, leading to an acidic pH.
What is the pH of a solution that has a concentration of hydrochloric acid equal to 0.001 M?
Remembwer pH is = the negative logarithm to base ten, of the hydrogen ion concentration . So with a concentration of 0.001 M The hydrogen ion concentration is 0.001 = 10^(-3) ph = -log(10)[H^+] pH = -log(10)10^-3 pH = -(-3) log(10)10 ( Remember log(10)10 = 1 ) pH = -(-3)(1) = --3 = 3 pH = 3
What is the pH when the hydrogen ion concentration is 2.0 x 10-3 M?
- log(2.0 X 10 -3 M) = 2.7 pH ======
What is the pH of a 1.6 10-3 M HNO3 solution?
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
What solution has a greater concentration of hydrogen ions a solution with a pH of 3 of a pH of 5 Explain?
1/103 = 0.001 M ========( pH 3 ) 1/105 = 0.00001 M ============( pH 5 ) As you see, a pH of 3 has a 100 times concentration of 5 pH ( 10 * 10 devalued ) This is the scale; logarithmic.
PH level when OH- equals 2.3 x 10-3 M?
The pH level when [OH-] equals 2.3 x 10^-3 M can be calculated using the equation: pOH = -log[OH-]. Given [OH-] = 2.3 x 10^-3 M, pOH = -log(2.3 x 10^-3) ≈ 2.64. Since pH + pOH = 14, pH = 14 - pOH = 14 - 2.64 ≈ 11.36.
What is the pH of a solution with H plus 2.3 10 -3?
5.0 x 10-3 pH = - log [H3O+] [H3O+] = 1 x 10^-pH pH = 2.3 [H3O+] = 1 x 10^(-2.3) = 5 x 10^(-3) M
What is the difference of substances with the pH of 2 3 and 6?
Substances with a pH of 2 are strongly acidic, pH of 3 is moderately acidic, and pH of 6 is slightly acidic. The lower the pH value, the higher the acidity of the substance. pH 2 is 10 times more acidic than pH 3, and 100 times more acidic than pH 6.
What is the pH of 1x10-3 H?
- log(1 X 10 -3 M H +) = 3 pH =====
What is the pH for 1.0 times 10 -3 m hcl?
The pH of a 1.0 x 10^-3 M HCl solution is 3.00. This is because HCl is a strong acid that dissociates completely in water to form H+ ions, leading to an acidic pH.
What is the pH when the hydronium ion concentration is 7.0 x 10-3 M?
pH = -log(0.007) = 2.16
What is the pH when the H plus equals 10-7 M?
3
What is the pH of resultant solution if solution with pH 3 and pH 8 are mixed?
To find the pH of the resultant solution, you can use the formula: pH = -log[H+]. Calculate the [H+] concentration for each solution using the pH values (pH 3 = 1.0 x 10^-3 M and pH 8 = 1.0 x 10^-8 M) and add them together. Then, convert the total [H+] concentration back to pH using the formula mentioned earlier.
