OH NewCars 101

What is the oxidation number of O in the ion OH-? - Socratic
In a hydroxide #(OH^-)# ion, we see that the total charge of the ion is #-1#. That means, the total sum of the oxidation numbers of the elements present in the ion totals out to be #-1#. The ion has one oxygen atom and one hydrogen atom. Hydrogen is less electronegative than oxygen, and so will possess its usual #+1# state.

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 ...

Balancing Redox Equations Using the Oxidation Number Method
Balancing a redox reaction requires identifying the oxidation numbers in the net ionic equation, breaking the equation into half reactions, adding the electrons, balancing the charges with the addition of hydrogen or hydroxide ions, and then completing the equation.

How can you tell the difference between an acid and a base ... - Socratic
In this case it is easiest to recognize the OH^- as a base (check: yes, it would accept a proton). That means the other compound on the right must be the acid. BOTH are "conjugates" of the original acid-base pair on the reactant side, so the original "acid" is H_2O (because the conjugate base is the OH^-) and the original base is the C_5H_5N.

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.

pH - Chemistry - Socratic
pH is a measure of hydrogen ion concentration. The pH scale was originated by Sorensen. He set 0 pH as the hydrogen ion concentration of a 1.0 molar solution of a strong monoprotic acid (like HCl).

What are the orders of "CV"^(+) and "OH"^(-) for the reaction "CV ...
Where #OH^-) and CV^+# are the concentration of them in M. We know that the concentration of NaOH is 0.1M or the #OH^- # concentration is 0.1M as 1 mol of NaOH contributes 1 mole of #OH^-# because it is a strong base. The equation for dissociation in water #"NaOH" + "H"_2"O" rightleftharpoons "Na"^+ + "OH"^-# Plug in the new found variable

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 ...

What is the [OH^-] in a solution of pH 3.00? - Socratic
#pOH=-log[OH^"-"]# Now if we take the Log from both sides of the #K_"w"# equation, we get: #log(1*10^(-14))=log([H_"3"O"]*[OH^-])# A mathematics rule tells us that multiplying inside the logarithm function is the same as adding these logarithms. Therefore we get #log(10^(-14))=log[H_"3"O"]+log[OH^-]# And now we can use the definitions of pOH ...