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What is the pH of a solution with a H3O of 7.9x10-11 M?
The pH of a solution with a H3O+ concentration of 7.9x10-11 M is approximately 10.1. This is because pH is calculated as -log[H3O+], so -log(7.9x10-11) ≈ 10.1.
What is the pH of a cleaning solution with a H3O 7.4 10-9 M H3O?
By definition: pH = -log[H3O+]So pH = -log(7.4*10-9) = 8.13
What is the pH of a solution whose h3o is 1 x 10 -5 m?
The pH of a solution with an H3O+ concentration of 1 x 10^-5 M is 5. This is because pH is defined as -log[H3O+], so by taking the negative logarithm of 1 x 10^-5, the pH is 5.
What is the pH of 4.3x10-8 M H3O?
- log(4.3 X 10 -8 M hydronium ) = 7.4 pH ------------- Indicates that hydronium to hydroxide concentrations are low, so slightly basic solution. About blood pH.
What is the pH of aqueous solution with the hydronium ion concentration H3O 210-14M?
The pH of the solution can be calculated from the hydronium ion concentration using the formula pH = -log[H3O+]. Plugging in the value given (H3O+ = 10^-14 M) gives a pH of 14.
What is the pH of a solution with a H3O of 7.9x10-11 M?
The pH of a solution with a H3O+ concentration of 7.9x10-11 M is approximately 10.1. This is because pH is calculated as -log[H3O+], so -log(7.9x10-11) ≈ 10.1.
What is the pH of a cleaning solution with a H3O 7.4 10-9 M H3O?
By definition: pH = -log[H3O+]So pH = -log(7.4*10-9) = 8.13
What is the pH of a solution whose h3o is 1 x 10 -5 m?
The pH of a solution with an H3O+ concentration of 1 x 10^-5 M is 5. This is because pH is defined as -log[H3O+], so by taking the negative logarithm of 1 x 10^-5, the pH is 5.
What is the pH of 4.3x10-8 M H3O?
- log(4.3 X 10 -8 M hydronium ) = 7.4 pH ------------- Indicates that hydronium to hydroxide concentrations are low, so slightly basic solution. About blood pH.
What is the pH of aqueous solution with the hydronium ion concentration H3O 210-14M?
The pH of the solution can be calculated from the hydronium ion concentration using the formula pH = -log[H3O+]. Plugging in the value given (H3O+ = 10^-14 M) gives a pH of 14.
What is the molarity of H3O plus in an aqueous solution of methanoic acid if its pH is 5.5?
The pH can be calculated using the formula pH = -log[H3O+]. Rearranging, [H3O+] = 10^(-pH). Therefore, [H3O+] = 10^(-5.5), which gives a molarity of approximately 3.16 x 10^(-6) M in the aqueous solution.
Calculate pH of H3Oplus equals 2.4EXP-10 M?
The pH of a solution can be calculated using the formula pH = -log[H3O+]. Plugging in the concentration of H3O+ given (2.4 x 10^-10 M), we get pH = -log(2.4 x 10^-10) = 9.62. Therefore, the pH of this solution is 9.62.
The ph of lemon juice at 298 k is found to be 2.32 what is the concentration oh H3O plus ions in the solution?
The concentration of H3O+ ions can be calculated using the formula pH = -log[H3O+]. Rearrange the formula to get [H3O+] = 10^(-pH). Plugging in the pH value of 2.32 gives a concentration of H3O+ ions of approximately 4.63 x 10^(-3) M.
What is the pH of a solution in which H3O plus equals 4.1 x 10-2 M?
1.39
What is the H3O concentration in a solution with a pH of 2.34?
pH = (by definition) = -log10[H3O+] , no matter what kind of acid,This inverted to:[H3O+] = 10-pH = becomes 10-2.9 = 1.3*10-3 mol/lNote: [H3O+] = concentration of hydronium ions (mol/l),which is the same as (or equivalent with) saying H+ ions concentration in water
What is hydronium-ion concentration of a solution when its pH is -0.120?
1/10 -0.120= 1.32 m h3o+==========
What is the H3O in 0048 M NaOH solution?
H3O+ concentration in a 0.048 M NaOH solution is 2.4 x 10^-12 M. This is because NaOH is a strong base that dissociates completely in water to produce Na+ and OH- ions, which react with any H3O+ ions to form water. As a result, the H3O+ concentration in such a solution is extremely low.
