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What is the pH of 3.0 M KOH?
Molarity is the concentration of a solution, defined as moles per unit volume. Where, Molarity = moles / volume In this case the molarity of the HCl solution is 0.03 M The pH of this is calculated by the equation below pH = - log [H+] Where [H+] is the concentration of hydrogen ions/ protons present in the solution. As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03 M Then the equation can be calculated (the minus sign is very important!) pH = - log 0.03 pH = 1.52 To summarise, Molarity of 0.03 M HCl solution is 0.03 M pH of 0.03 M HCl solution is 1.52
Calculate the pH of 0.01m hcl?
HCl is a strong acid, so we assume that it completely breaks up into ions in solution. HCl ----> H+ & Cl- if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl- pH = -log [H+] pH = -log 0.01 pH = 2
When the H in a solution is 1.7 109 M what is the pOH?
To find the pOH of a solution when the H concentration is 1.7 x 10^-9 M, you can first calculate the pH using the formula: pH = -log[H+]. Then, you can find the pOH by subtracting the pH from 14, since pH + pOH = 14 in water. So, if the H concentration is 1.7 x 10^-9 M, the pH is 8.77, and the pOH is 14 - 8.77 = 5.23.
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
What is the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
What is the pH of 3.0 M KOH?
Molarity is the concentration of a solution, defined as moles per unit volume. Where, Molarity = moles / volume In this case the molarity of the HCl solution is 0.03 M The pH of this is calculated by the equation below pH = - log [H+] Where [H+] is the concentration of hydrogen ions/ protons present in the solution. As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03 M Then the equation can be calculated (the minus sign is very important!) pH = - log 0.03 pH = 1.52 To summarise, Molarity of 0.03 M HCl solution is 0.03 M pH of 0.03 M HCl solution is 1.52
Calculate the pH of 0.01m hcl?
HCl is a strong acid, so we assume that it completely breaks up into ions in solution. HCl ----> H+ & Cl- if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl- pH = -log [H+] pH = -log 0.01 pH = 2
When the H in a solution is 1.7 109 M what is the pOH?
To find the pOH of a solution when the H concentration is 1.7 x 10^-9 M, you can first calculate the pH using the formula: pH = -log[H+]. Then, you can find the pOH by subtracting the pH from 14, since pH + pOH = 14 in water. So, if the H concentration is 1.7 x 10^-9 M, the pH is 8.77, and the pOH is 14 - 8.77 = 5.23.
What is the pH of a 0.0110 M solution of Ba OH2?
The pH of a 0.0110 M solution of Ba(OH)2 can be calculated by finding the hydroxide ion concentration, which is double the concentration of the Ba(OH)2 solution. Therefore, [OH-] = 2 * 0.0110 M = 0.0220 M. From this, you can calculate the pOH using the formula -log[OH-], and then convert pOH to pH using the relation pH + pOH = 14.
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
What is the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
If the pH of a solution is 10.7, what would the pOH be?
The pOH is 6,4.
What is the pH of 260M HCl?
.260 M of HCL, not 260 More than likely correct, but, - log(0.260 M HCl) = 0.6 pH ----------- ( pH can be below 1 )
What is the pH of a solution with a oh of 3.31 00000000 M?
The pH of a solution can be calculated using the formula pH = 14 - pOH. Given that the pOH is 3.31, we can subtract this value from 14 to find the pH. In this case, the pH of the solution would be approximately 10.69.
What is the pH of a 0.001 M of HCl solution?
its PH is 3
How do you calculate OH- with a ph of 1.12?
To calculate the concentration of hydroxide ions (OH-) from a given pH value, you can use the formula: [OH-] = 10^(-pH). For a pH of 1.12, the concentration of hydroxide ions would be [OH-] = 10^(-1.12) = 0.079 moles per liter.
What is the pH of a 10-5 m of koh solution?
The pH of a 10^-5 M KOH solution would be around 9. For a given concentration of a strong base like KOH, the pH can be calculated using the formula pH = 14 - pOH. Given that pOH = -log[OH-] and [OH-] = 10^-5 M in this case, pOH = 5. Therefore, pH = 14 - 5 = 9.
