0
What is the hydronium ion concentration of a solution at 298 K whose hydroxide ion concentration is 1 x 10-8 A 1 x 10-6 B 1 x 10-7 C 1 x 10-8 x D 1 x 10-14?
What else can I help you with?
What is the hydronium ion concentration of a solution at 298 K whose hydroxide ion concentration is 1 x 10-8?
The hydronium ion concentration can be found using the formula Kw = [H3O+][OH-], where Kw is the ion product constant (1 x 10^-14 at 298 K). Given the hydroxide ion concentration as 1 x 10^-8, the hydronium ion concentration is 1 x 10^-6 M.
What is the hydroxide ion concentration of a solution whose pH is 12.40?
The hydroxide ion concentration can be calculated using the formula [OH-] = 10^-(14-pH). Thus, for a solution with pH 12.40, the hydroxide ion concentration would be 10^-(14-12.40), which is equal to 2.51 x 10^-2 M.
What is the concentration of the hydroxide ions of a solution whose pH is 4.0?
The concentration of hydroxide ions (OH-) in a solution with a pH of 4.0 is 1 x 10^-10 mol/L. This value can be calculated using the relationship between pH and pOH (pOH = 14 - pH), and then using the formula for the concentration of hydroxide ions in water at a given pOH.
What is the pH of a solution whose hydronium ion concentration is 5.03 and nbsp and acute and nbsp10-1 M?
The pH of a solution can be calculated using the formula pH = -log[H+]. Given that the hydronium ion concentration is 10^-1 M, the pH of the solution is pH = -log(10^-1) = 1. So, the pH of the solution is 1.
What is pH of the solution whose hydroxide in concentration is 4?
The pH of a solution is a measure of its acidity or basicity. To calculate the pH from the hydroxide concentration, you would first need to convert the concentration to a pOH value using the equation pOH = -log[OH-]. Then, you can calculate the pH using the relationship pH + pOH = 14.
Which term is applied to an aqueous solution whose hydrogen ion concentration H plus is less than its hydroxide ion concentratio OH?
The term applied to an aqueous solution with a hydrogen ion concentration (H+) lower than the hydroxide ion concentration (OH-) is basic or alkaline. This indicates that there are more OH- ions present, making the solution basic on the pH scale.
Weak acid or base whose color depends on hydronium ion concentration?
An indicator is a weak acid or base that changes color depending on the hydronium ion concentration in a solution. The color change occurs due to a shift in the equilibrium between the protonated and deprotonated forms of the indicator molecule in response to changes in pH. Common indicators include phenolphthalein, litmus, and bromothymol blue.
What is the oh- of a soultion whose pH is 10?
The concentration of hydroxide ions (OH-) can be calculated from the pH using the formula: [OH-] = 10^(14 - pH). In this case, for a solution with a pH of 10, the concentration of OH- ions would be 10^(-4) M.
What is the name of a solution whose concentration of solute is equal to the maximum concentration that is predicted from the solute's solubility?
A solution whose concentration of solute is equal to the maximum concentration predicted from the solute's solubility is called a saturated solution. In a saturated solution, the solute is in equilibrium with its undissolved form, meaning no more solute can dissolve at that specific temperature and pressure.
Gas whose aqueous solution is basic?
Ammonia gas when dissolved in water produce Ammonium hydroxide so its solution is basic.
Difference between primary standard solution and a secondary standard solution in acid-base titration?
primary standard solution is prepared by direct measurements of the mass of solute and the volume of solution.whereas, a secondary standard solution is a solution whose concentration can't be determined directly from weight of solute and volume of solution, the concentration must be determined by analysis of the solution itself.
Describe how water moves during?
From areas of higher concentration (of water) to lower concentration (of water) - ie it fills the space. That would mean that it would flow from a solution whose concentration of solute is higher to one where the solute concentration is lower.
