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If the (H plus ) in a solution increases the (OH-) must decrease?
Yes, it is correct.
How does the concentration of OH- ions change if its pH changes from 8 to 13?
The pH increasing from 8 to 13 means the solution is becoming more basic. As pH increases, the concentration of OH- ions also increases since pH is a logarithmic scale that measures the concentration of hydrogen ions. So, in this case, the concentration of OH- ions would increase as the pH increases from 8 to 13.
Do buffers release H plus ions when pH increases?
Yes, buffers can release or absorb H+ ions to help maintain a relatively stable pH when an acid or base is added. When the pH of a solution increases, some buffers can release H+ ions to counteract the change and prevent a drastic shift in pH.
Does salt dissociates into H plus and OH- in solution?
No, salt (such as NaCl) does not dissociate into H+ and OH- ions in solution. Salt dissociates into Na+ and Cl- ions. It is only certain substances, like acids and bases, that can dissociate into H+ and OH- ions in solution.
Why does a basic solution contain some H ions?
It is not to do with buffers. If you take pure water at 25°C, it dissociates: H2O ↔ H+ + OH- ( I use H- instead of H3O+ for simplicity) You ask about bases: If you add a base, such as NaOH to the water, you introduce a high concentration of OH- ions to the water. This causes the dissociation equilibrium of the H2O to move to the left. ( In accordance with Le Chettellier) But the re-association of the H+ and OH - from the water is not complete - there are always some H+ ions dissociated This is determined by the equation: [H+] [OH-] = 10^-14 You can see this from the pure water where [H+] and [OH-] are both 1*10^-7M - the equation is satisfied Now on adding the base, the [OH-] increases to 5*10^-3M , What is [H+] in this solution: [H+] = 10^-14 / (5*10^-3) = 2*10^-12M There will be a reducing concentration of H+ as [OH-] increases, but always some H+ present The converse happens with an acid solution You add acid, say HCl to the water so that [H+] = 5.10^-3 [OH-] = (10^-14)/ (5*10^-3) = 2*10^-2M Even in the acid solution there will be some OH- ions present.
If the (H plus ) in a solution increases the (OH-) must decrease?
Yes, it is correct.
Which ion is donated by an acid when added to water OH- OH plus H- or H plus?
H+ or a proton.
What is the net ionic equation of Na plus plus OH- plus H plus plus Cl- H2O plus Na plus plus Cl-?
The net ionic equation for the given reaction is H+ (aq) + OH- (aq) → H2O (l)
What happens in a buffer when the level h plus ions in solution increases?
It accepts H+ ions.
What is represented by H2O H plus plus OH?
The representation H2O H plus plus OH signifies the dissociation of water molecules into hydronium ions (H+) and hydroxide ions (OH-) in aqueous solution. This is the auto-ionization of water where some water molecules act as both acids (donating H+ ions) and bases (accepting H+ ions). The concentration of H+ and OH- ions in pure water is equal at 10^-7 M.
If an acid is added to a solution does the H plus concentration increase or decrease?
It increases.
What is H plus and OH?
Water , This is a poorly written chemical equation for the formation/dissociation of water. H^(+) + OH^(-) H2O(l)
What does H plus and OH- stand for?
H plus and OH negative are ions of hydrogen and hydroxide in their dissolved states. When a compound is broken down, it is broken down into it's ions, which will each have a charge.
Lower concentrations of H plus ions than pure water basic acidic or polarity?
Lower concentrations of H+ ions indicate a basic solution. Pure water has a neutral pH, so any solution with a lower concentration of H+ ions than pure water would be considered basic. Acidity increases as the concentration of H+ ions in a solution increases.
H plus Cl- plus Na plus OH- Na plus Cl- plus H2O is?
Hydrochloric acid and sodium hydroxide yield salt and water H+ + Cl- + Na+ + OH- --> Na+ + Cl- + H2OComment:In solutions you better leave unchanged ions ( Cl- and Na+) out of the balanced equation: called to be 'tribune ions' (people on the tribune don't take part in the 'match'):H+ + OH- --> H2O This looks simpler than: H+ + Cl - + Na + + OH- --> Na + + Cl - + H2O
When equivalent amounts of h plus and OH- have reacted in titration?
Endpoint
What substance neutralizes H plus?
The ion H+ is neutralized adding a ionic substance containing the in OH-.
