How to you convert between pH, pOH, [H+] and [OH-]? - Socratic
Here's a concept map that shows how to get from any of these to the other. [Really, the only things you need to remember are:

How do you calculate the pH of a solution when given the OH ...
The pH + pOH = 14 The pOH = -log[OH-] The pH is measure of acidity of a solution whereas the pOH is a measure of basicity of a solution. The two expressions are opposites expressions. As the pH increases the pOH decreases and vice versa. Both values equal 14. To convert a concentration of into pH or pOH take the -log of molar concentration of the hydrogen ions or the molar concentration of the ...

As the H^+ in a solution decreases, what happens to the OH ... - Socratic
As the [H^+] ion decreases the [OH^-] ion increase. The Keq for water is 10^-14 This means that the Hydrogen ion concentration times the Hydroxide concentration must always be the same 10^-14 [H^+] xx [OH^-] = 10^-14 This means that the two ions are inversely proportional. If one goes up the other goes down. At the neutral point of water, both the Hydrogen ion and Hydroxide ion are equal at 10 ...

What is the balanced chemical equation that describes the ... - Socratic
The equation is "Mg(OH)"_2"(s)" ⇌ "Mg"^"2+""(aq)" + "2OH"^"-""(aq)". > "Mg(OH)"_2 is a strong base. "Mg" is a Group 2 Metal, so it form "Mg"^"2+" ions. Each ion pairs up with two "OH"^"-" ions to form the neutral compound, "Mg(OH)"_2. Magnesium hydroxide is "insoluble", so only a small amount it goes into solution. But every bit that goes into solution dissociates into "Mg"^"2+" ions and "OH ...

Oxidation Numbers - Chemistry - Socratic
Oxidation numbers are used to track how many electrons are lost or gained in a chemical reactions. Assigning these numbers involves several rules: Free atoms (H2) usually have an oxidation number of 0, monoatomic ions (Cl-) are usually equal to their charge, and polyatomic ions have several governing principles.

Conjugate Acid and conjugate Base for the reaction NH3 - Socratic
Well look at defining reaction.... "Acid + Base "rightleftharpoons" Conjugate base + conjugate acid" And so we got.... underbrace(NH_3(aq))_"base" + H_2O(l ...

What are the spectator ions in #Na^+ + OH^- + H^+ + Cl^- -> H_2O - Socratic
And when we get the reactants into solution, [Na{(OH)_2}_6]^+, remains substantially unchanged during the reaction; it is a SPECTATOR that cheers on the bond-making reaction between the ACTIVE hydroxide and protium ions..... H_3O^+ + HO^(-) rarr 2H_2O(l) If you have further queries fire away, because this is a very important formalism to ...

Conjugate Acids and Conjugate Bases - Chemistry - Socratic
HCO₃⁻ + H₂O → H₂CO₃ + OH⁻ base + acid → Conj A + Conj B. We see that HCO₃⁻ becomes H₂CO₃. It has one more H atom and one more + charge (-1 + 1 = 0). So H₂CO₃ is the conjugate acid of HCO₃⁻. The H₂O becomes OH⁻. It has one less H atom and one more – charge. So OH⁻ is the conjugate base of H₂O.

Nucleophile vs. Base Strength - Organic Chemistry - Socratic
Examples are: RO⁻, OH⁻, RLi, RC≡C:⁻, and NH₂⁻. Strong Bases/Poor Nucleophiles. Some strong bases are poor nucleophiles because of steric hindrance. Examples are t-BuO⁻, t-BuLi, and LiN[CH(CH₃)₂] Weak Bases/Good Nucleophiles. I⁻ is a weak base, but it is a good nucleophile because the large electron cloud is highly polarizable.

What is the [OH^-] in a solution that has a [H_3O]=1.0*10^-6 M ...
The answer can be obtained one of two ways: #color(red)("Use the auto-ionization constant of water equation, Kw:"#