What is the concentration of the hydroxide ion given that the concentration of the hydronium ion is 1.5x10-5M?
1 x 10-9
In neutral solutions, [H3O+] = [H2O].In bases, [OH-] = [H3O+].In bases, [OH-] is greater than [H3O+].In acids, [OH-] is greater than [H3O+].In bases, [OH-] is less than [H3O+].
NaO sodium oxide
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Weigh 10g of the given sample and dissolve it in 100ml of water, it forms a 10% solution of that sample.
You can do it with a pH probe, or, if you are given the Ka value for phosphoric acid, you can do some math and figure it out.
4.33 X 10^11
pH is not a measure of how strong an acid is. pH is a measure of the concentration of hydronium ions in a solution, which is dependent on both the strength of the acid or base and its concentration in a given solution.
You will need Kw to determine the concentration of hydrogen ions and You will need the formula pH = -log[H+]
In a solution (in this case, sand), a Ph rating of 7 or "neutral" is given if the number of Hydronium ions is equivalent to the number of Hydroxide ions.
The number of molecules in a given volume of solution depends on the concentration of the solute. Because the concentration is not provided, this question has too little information to answer.
The pH of a solution with a hydronium ion concentration of 2.5 micro moles per liter can be calculated using the following formula: [ \small \text{pH} = -\log(\text{[H}_3\text{O}^+]) ] Given the concentration of hydronium ions, we can plug in the value: [ \small \text{pH} = -\log(2.5 \times 10^{-6}) ] Calculating this: [ \small \text{pH} = -\log(0.0000025) = 5.60 ] Therefore, the pH of the solution is approximately 5.60
A solution with a greater concentration of hydrogen ion (H+) than hydroxide ion (OH-) is an acid while the inverse would be a base.
Hydrogen gas is given out when sodium hydroxide reacts with a metal.
pH is just the -log of the concentration of hydronium ion, and pOH is the same but for the concentration of hydroxide ion. The following equations are useful for solving this type of problem. pH=-log[H30+] pOH=14-pH pOH=-log[OH-] The inverse of log is 10^x, so [H3O+]=10^-pH
In neutral solutions, [H3O+] = [H2O].In bases, [OH-] = [H3O+].In bases, [OH-] is greater than [H3O+].In acids, [OH-] is greater than [H3O+].In bases, [OH-] is less than [H3O+].
That really depends upon the type of tea you have brewed. There are a number of interesting compounds present in tea, the concentration of which vary with type, variety and blend. The nature of the water you brew the tea with will also have a profound effect on the extraction of these compounds. The cup of tea I have in front of me has a pH of 6.2. Given that pH = -log10 [H30+], the hydronium ion content of this is 6.31 x 10^-7 mol dm-3 Hope that helps. Richard
In theory any pH is possible, especially at elevated temperatures where pure water decreases in pH because of increased ionisation (but it is still neutral, neither acidic nor alkaline). However, does anything dissolve at sufficiently high concentration, and ionise sufficiently at that concentration, to achieve any given pH? In practice there are limitations. At pH 15, hydrogen ion concentration is 10^-15. That makes hydroxide ion concentration 10^1 - 10M sodium hydroxide in theory would have a pH of 15.