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CH 3COOH (aq) +OH − (aq) → CH 3COO− (aq) +H 2O(l) Notice the 1:1 mole ratio that exists between acetic acid and sodium hydroxide (written as hydroxide ions). This means that, in order to get a complete neutralization, you need equal numbers of moles of each compound.

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Question #a721d - Socratic

pH = 1.61151 OH^- = 4.08797 * 10 ^-13M HF = 0.855538M H^+ = 0.024462M F^- = 0.024462M HF + H_2O = H_3O^+ + F^- We can find the concentration of H^+ or H_3O^+ by three ways One is by the ICE table (but this is a 5% rule) and the other is square root which is absolutely correct and the other is Ostwald's law of dillution Let's set up an ICE table. color (white) (mmmmmmmm)"HF" + "H"_2"O" ⇌ "H ...

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Question #70577 - Socratic

Here's what I got. Start by writing the balanced chemical equation for this neutralization reaction. Since sodium hydroxide is a strong base that dissociates completely in aqueous solution, you can represent it by using the hydroxide anions, "OH"^(-) "HA"_text((aq]) + "OH"_text((aq])^(-) -> "A"_text((aq])^(-) + "H"_3"O"_text((aq])^(+) Now, you have 1:1 mole ratios across the board, you can say ...

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Question #750c8 - Socratic

Here's what I got. The problem wants you to use the base dissociation constant, K_b, of ammonia, "NH"_3, to determine the percent of ammonia molecules that ionize to produce ammonium cations, "NH"_4^(+), and hydroxide anions, "OH"^(-). As you know, ammonia is a weak base, which means that it does not ionize completely in aqueous solution. Simply put, some molecules of ammonia will accept a ...

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Question #71b91 - Socratic

Since water is in excess, "67.7 g MgO" are needed to produce "98.0 g Mg(OH)"_2. Balanced equation "MgO(s) + H"_2"O(l)"rarr"Mg(OH)"_2("s")" Moles magnesium hydroxide Start with the given mass of "Mg(OH)"_2 and convert it to moles by dividing by its molar mass ("58.319 g/mol"). Since molar mass is a fraction, "g"/"mol", we can divide by multiplying by the reciprocal of the molar mass, "mol"/"g ...

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Question #d6b18 - Socratic

We want the standard enthalpy of formation for Ca (OH)_2. Thus, our required equation is the equation where all the constituent elements combine to form the compound, i.e.: Ca +H_2+O_2->Ca (OH)_2 Let us now write down the given equations: [The first equation mentioned is incorrect, and so I have revised it.] (1) 2H_2 (g) + O_2 (g)->2H_2O (l) and DeltaH_1=-571.66 kJmol^-1 (2) CaO (s) + H_2O (l ...

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Question #9be9c - Socratic

The correct answer is a) hydroxide, carbonate, and hydrogen carbonate. Alkalinity is another word for basicity (the concentration of hydroxide ions). a) Hydroxide ions OH⁻ are the strongest base you can have in water. Carbonate ions and hydrogen carbonate ions also react with water to form hydroxide ions. CO₃²⁻ + H₂O ⇌ HCO₃⁻ + OH⁻ HCO₃⁻ + H₂O ⇌ H₂CO₃ + OH⁻ b ...

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Question #18488 - Socratic

The degree of dissociation sf (alpha=0.0158) sf (K_b=2.51xx10^ (-6)color (white) (x)"mol/l") Triethyamine is a weak base and ionises: sf ( (CH_3)_3N+H_2Orightleftharpoons (CH_3)_3stackrel (+) (N)H+OH^-) For which: sf (K_b= ( [ (CH_3)_3stackrel (+) (N)H] [OH^ (-)])/ ( [ (CH_3)_3N])) Rearranging and taking -ve logs of both sides we get the ...

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Question #370a7 - Socratic

The sodium ions remain in solution as spectator ions. If XS sodium hydroxide is added the precipitate redissolves to give the soluble plumbate (II) ion. A simple way of writing this is: (chemguideUK) Ammonia solution can't do this as the concentration of OH^ (-) ions is not high enough.

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Question #889ec - Socratic

Explanation: < Since the molarity of either acid is the same, the moles of each acid are equal. That means the difference between their pH is determined solely on which acid dissociates more. Since the strong acid dissociates more (releases more #H^+# ions), it will have a lower pH. = Since both acids are monoprotic (they only release one hydrogen) they will both take the same amount of #OH ...