when is x negligible

[005199302]

When can we assume that [OH-]=[H30+]? Is it when Kw is less than 10^3?

[Parth Mungra]

x is negligible when the acid/base reacting with water is weak, meaning very little will dissociate into ions. Therefore, we consider this change in concentration (x) from initial to final to be so small that it can be negated.

[anthony_trieu2L]

[OH-] is equal to [H30+] when the pH of the solution is neutral. Kw is always 1 x 10^-14 at 25 C.

[Brandon Mo 4K]

You can also tell if x is negligible by seeing if the value of x is less than 5% of the initial molarity of the reactant after using the approximation.

[Aria Soeprono 2F]

Also, just something to keep in mind, is that if you have already solved the problem using the shortcut (when you assume x to negligible), Lavelle said that the general rule is anytime x is less than 5% of the initial value, then it is safe to assume an approximation to 0.

[Marina Gollas 1A]

Here something that another student said in this forum that helped me understand. :)
"The reason that you can do an approximation where you "ignore" the x in the denominator [of the equation to find x when you complete the Ice tables], is because if the K value is smaller than 10^-3, then the x when multiplied out by this k value will be very negligible [since it's like 3-0.00000999, in which case the result is still quite close to 3, so there was barely any significance with this minimal change in the value]. So, instead of going through the whole process and doing the quadratic formula in this specific case, it is much easier and still pretty accurate to approximate the value of x in the denominator to be equal to zero."

[LedaKnowles2E]

X is negligible when x is less than 5% of the initial concentration, or when K is less than 10^-3.

[Nathan Mariano 2G]

X is negligible when the equilibrium constant/acid dissociation constant (Ka)/base dissociation (Kb) constant is smaller than 10^-3. Also, as repeated above, X is negligible when it is less than 5% of the initial concentration.