Which of these statements are true for a neutral, aqueous solution at 25 °C? [ht] = [OH] pH = 7.00 pOH = 7.00 Which of these statements are true for a neutral, aqueous solution regardless of temperature? pOH = 7.00 [H] = [OH) pH = 7.00 Explain your reasoning: This ungraded area will provide insight to your instructor 500 Characters remaining

If pH = 7, the solution is said to be neutral.

If pH > 7, the solution is basic in nature.

If pH < 7, the solution is acidic in nature.

1)

At 25°C, Ionic product of water (Kw) = 1.0*10-14  

For water,Kw = [H+] * [OH?????-] =  1.0*10-14  

For water, we know that   [H+] = [OH?????-]

[H+]2 =  1.0*10-14  

    [H+] =√(1.0*10-14)

    [H+] =1.0*10-7 M

Similarly   [OH?????-] =1.0*10-7 M

pH is the negative logarithm of Hydronium ion concentration.

pH = -log[H+] = -log(1.0*10-7  M)

pH = 7

Similarly pOH is the negative logarithm of hydroxyl ion concentration.

pOH = -log[OH?????-] = -log(1.0*10-7 M) = 7

For neutral aqueous solution at 25°C, pH = 7, pOH = 7 and concentration of Hydronium ions is equal to Concentration of hydroxyl ion.

2)

For neutral solution, regardless of temperature,

[H+] = [OH?????-]

But pH may or may not equal to 7. Similarly pOH also may or may not be 7. Here pH value depends on temperature.

If temperature is increased, the dissociation of water increases. Hence the concentration of Hydronium ions or concentration of hydroxide ions increases. Hence may be pH is either < 7 or > 7.