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To find the hydronium ion concentration from pH, set base 10 to the negative power of the pH. Here that corresponds to 10 to the power of -8.75
The answer is 0.000000002 or 2x10^-9
Although this response is correct in saying that concentration and pH are based on sets of base 10; however, it is incorrect in it's response.
From pH--> [H30]
-log(pH)
From [H30]---> pH
10^(-pH)
Wiki User
∙ 13y ago
Wiki User
∙ 16y agoph=-log[H+] so -log [H+]=8 then [H+]=10^(-8) mole/lit
Wiki User
∙ 14y agoTo find H+ concentration type into calculator: 10x (shift log), and then type the pH value for x
So 10-8 = 1x10-8
Wiki User
∙ 9y agoTo find H+ concentration type into calculator: 10x (shift log), and then type the pH value for x
So 10-8 = 1x10-8
Wiki User
∙ 11y agoHydroxide concentration.
1/108
= 1 X 10 -8 M
==========
Wiki User
∙ 13y ago0.000001 molar
Wiki User
∙ 12y ago10^-6
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A hydroxide ion is indicated by?
As a chemical ion it is 'OH^-'. As in sodium hydroxide NaOH. A pH indicator will shown it as pH 8 to 12' depending on the ionic strength. A Universal Indicator will colour 'blue/violet/indigo'.
A solution has 0.000001 moles of hydroxide ions per liter - what is the pH of the solution?
pH is 8
Electron dot structure of the hydroxide ion?
The picture of the lewis dot structure for hydroxide can be found in the link below( look in the RELATED LINKS tab below )qqq
Does a phenolphthalein indicator remain clear in an acid?
It does turn orange at exceptionally low pH (below 0), but that corresponds to a fairly high (greater than 1 molar) concentration of a strong acid. Between pH 0 and pH 8 or so it's colorless, so it's not particularly useful as an indicator for most acids. Somewhere between pH 8 and pH 10 it begins to turn a characteristic pink color. Above pH 12 the color fades again.
What is The pH of a 0.0000001 M solution of hydrogen chloride in water?
No It Is Not '8':Assuming the concentration of the strong monoprotic acid(eg. HCl) in the solution = 10-8 mol/L and this has been added to pure water, which already contains 10-7 mol/L H+ions, the total concentration of H+ions can be reasonably well approximated by adding up these two values, so [H+]total will be 1.1*10-7 .As pH is defined at the negative of the logarithm of the concentration of hydrogen ions the outcome is 6.96 rounded to pH = 7, which is of course much better than the (often MIScalculated) pH value 8, because adding an ACID always decreases the pH value, NEVER increased to 'above' 7!And also, assuming the concentration of a strong monoprotic base NaOH in the solution = 10-8 mol/L and this has been added to pure water, which already contains 10-7 mol/L OH- ions, the total concentration of OH-ions can be reasonably well approximated by adding up these two values, so [OH-]total will be 1.1*10-7 . So pH = 14 - pOH = 7.04. This is the same parallel story for base and acid.
What is the difference between a pH of 6 and a pH of 8 in H plus concentration terms?
The difference between a pH of 7 and a pH of 8 are as follows:A pH of 7 means the concentration of [H+] is 10-7.A pH of 8 means the concentration of [H+] is 10-8.Therefore, a substance with a pH of 8 has 1/10th the concentration of hydrogen ions that a substance with a pH of 7.
A hydroxide ion is indicated by?
As a chemical ion it is 'OH^-'. As in sodium hydroxide NaOH. A pH indicator will shown it as pH 8 to 12' depending on the ionic strength. A Universal Indicator will colour 'blue/violet/indigo'.
By what factor does the hydroxide ion concentration change if pH solution changes from 10 to 8?
pH 10 means [H+] = 1x10^(-10) mol dm-3 (0.0000000001 mol dm-3) pH 8 means [H+] = 1x10^(-8) mol dm-3 (0.00000001 mol dm-3) So basically it's changed by a factor of 100.
What is the pH pOH andOH- of a solution that has a hydronium ion concentration of 8.0 times 10 negative 6 M?
Important Notice: pH = negative value of the log10 of the hyronium concentration, which is very low, mostly
Change of a solution that goes from a pH 6 to a pH 8?
The easiest definition of pH, useful at the ranges you mention, is the concentration of hydrogen ions (or univalent donors) in a solution. pH units were defined to use a log base 10 scale rather than a linear scale in order to conveniently represent an enormous range of ion concentrations. Each unit change of pH reflects a 10-fold change of ion concentration. Increasing pH was arbitrarily chosen to represent decreasing hydrogen ion concentration. Hence pH6 to ph8 is a 100x decrease in hydrogen ion concentration.
If you have 14 ml of acidic solution with pH 3 how many ml of solution with pH 8 will you need to add to make the solution pH 7?
You would need to add enough of the alkaline solution to make the total volume 14 litres. The pH of a solution is a measure of the concentration of the hydrogen ion. In fact it is the logarithm of the reciprocal of the hydrogen ion concentration. Water ionizes to give one hydrogen ion per 10 million molecules so the pH is log(10,000,000)=7. The pOH (alkalinity) is obtained by taking the pH away from 14. So pH 8 is equivalent to pOH 6. The pOH is the logarithm of the reciprocal of the hydroxide ion concentration. To achieve neutrality the number of hydrogen ions must balance the number of hydroxide ions. The difference between the pH of the acid solution and the pOH of the alkaline solution is 3. This tells us that the acid is 10 to the power of 3 times i.e. a thousand times more concentrated than the alkaline solution. Thus the acid needs to be diluted to one part in a thousand with the alkaline solution.
When the concentration of hydrogen ions increases the pH number of a solution does what?
raises the pH Edited by Dr.J.: Are you kidding me? Raising the H3O+ concentration does NOT raise the pH, it LOWERS the pH. I can't believe that 8 people actually found this incorrect answer to be useful.
How great a differences is there in thr hydrogen ion concentration between a pH of 6 and a pH of 8?
im sorry i dont quite know the answer thatswhy im asking
What is the pH of a solution in which the hydrogen ion concentration is 5.1x0.000000010M?
pH+pOH=14 -> pH+5.010=14 -> pH= 8.99
What is the H3O plus ion concentration of a solution whose pH is 11?
The lower the value/number of pH means the hydrogen ion concentration is greater. Remember pH = -log(10)[H^+] Its mathematical inverse is [H^+] = 10^(-pH) So substituting the numbers 7.6 & 9.4 [H*+] = 10^(-7.6) = 2.51188... x 10^(-8) [H^+] = 10^(-9.4) = 3.98107... x 10^(-10) NB the coefficients may be larger, but the powers of '10' makes 9.4 < 7.6
How does the concentration of OH- ions change if its pH changes from 8 to 13?
As pH increases H+ ions concentration decreases means OH- ions concentration increases . If pH increases from 8 to 13 , OH- ions concentration increases.
What is the hydronium ion concentration of a solution at 298 K whose hydroxide ion concentration is 1 x 10-8?
[H3O+]*[OH-]=1.0*10-14 at 298K ,so [H3O+] = 1.0*10-14 / [OH-] = 1.0*10-14 / 1.0*10-8 = 1.0*10-6 mol/L
