Balance the following equations: (d) KOH(aq) + H 3 PO 4 (aq) → K 3 PO 4 (aq) + H 2 O(l)

Hey everyone. We're asked to balance the given chemical reaction first. Let's go ahead and count the number of atoms we have on both sides. Starting off with our react inside. We have one of nickel, one of hydrogen, one of nitrogen And three of oxygen. Looking at our product side, we have one of nickel as well, two of hydrogen, three of nitrogen and nine of oxygen only. Our nickel is balanced out. Let's first start off by balancing out our hydrogen. So if we add a coefficient of two prior to our nitric acid, we then are able to change our hydrogen into two, our nitrogen into two as well, And our oxygen's into six. Since we still need to change our nitrogen and oxygen's, this means we have to change The coefficient that we just inputted, which is R two. So instead of two, we can then go ahead and input a four prior to our nitric acid. And when we do that, we change our hydrogen into four, Our nitrogen into four as well. And our oxygen's into 12. Now that we've done this, we can adjust accordingly and look at our product side, we can add a coefficient of two prior to our water. And when we do this, we end up with four of hydrogen and our oxygen's changed from 9 to 10. Lastly, all we need to do is fix our nitrogen and our oxygen's and we can do that by fixing our nitrogen dioxide. So when we add a two prior to nitrogen dioxide, We end up with four of nitrogen And 12 of oxygen. So our balanced chemical reaction is going to be as such. So I hope this made sense and let us know if you have any questions.

Ch.3 - Chemical Reactions and Reaction Stoichiometry

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Brown 14th Edition

Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 14d

Chapter 3, Problem 14d

Balance the following equations: (d) KOH(aq) + H₃PO₄(aq) → K₃PO₄(aq) + H₂O(l)

Verified step by step guidance

Identify the reactants and products in the chemical equation: Reactants are KOH and H_3PO_4, and products are K_3PO_4 and H_2O.

Write the unbalanced chemical equation: KOH + H_3PO_4 \rightarrow K_3PO_4 + H_2O.

Balance the potassium (K) atoms: There are 3 K atoms in K_3PO_4, so place a coefficient of 3 in front of KOH.

Balance the phosphate (PO_4) groups: There is 1 PO_4 group on both sides, so they are already balanced.

Balance the hydrogen (H) and oxygen (O) atoms: Adjust the coefficient of H_2O to balance the remaining H and O atoms.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Coefficients are used to adjust the number of molecules or formula units to achieve balance.

Acid-Base Reactions

The reaction between KOH and H3PO4 is an example of an acid-base reaction, where KOH acts as a base and H3PO4 as an acid. In such reactions, the base donates hydroxide ions (OH-) while the acid donates protons (H+), leading to the formation of water and a salt. Understanding the properties of acids and bases is crucial for predicting the products of these reactions.

Ionic Compounds and Solubility

The products of the reaction, K3PO4 and H2O, involve ionic compounds. K3PO4 is a soluble salt formed from potassium ions (K+) and phosphate ions (PO4^3-). Knowledge of solubility rules helps determine whether the products will remain in solution or precipitate out, which is important for understanding the overall reaction dynamics.

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Related Practice

Textbook Question

Balance the following equations:

(a) CaS(s) + H₂O(l) → Ca(HS₂)₂(aq) + Ca(OH)₂(aq)

(b) NH₃(g) + O₂(g) → NO(g) + H₂O(g)

(d) FeS₂(s) + O₂(g) → Fe₂O₃(s) + SO₂(g)

Textbook Question

Balance the following equations: (a) CF₄(l) + Br₂(g) → CBr₄(l) + F₂(g) (b) Cu(s) + HNO₃(aq) → Cu(NO₃)₂(aq) + NO2(g) + H₂O(l)

Textbook Question

Balance the following equations: (c) MnO₂(s) + HCl(aq) → MnCl₂(s) + H₂O(l) + Cl₂(g)

Textbook Question

Write balanced chemical equations corresponding to each of the following descriptions: (a) Potassium cyanide reacts with an aqueous solution of sulfuric acid to form hydrogen cyanide gas. (b) When an aqueous solution of ammonium nitrite (NH₄NO₂) reacts with an aqueous solution of potassium hydroxide, ammonia gas, water and metal nitrate is formed. (c) When hydrogen gas is passed over solid hot iron(III) oxide, the resulting reaction produces iron and gaseous water. (d) When liquid ethanoic acid (CH₃COOH) is combusted, carbon dioxide and water are formed.

Textbook Question

Write balanced chemical equations to correspond to each of the following descriptions: (a) When sulfur trioxide gas reacts with water, a solution of sulfuric acid forms. (b) Boron sulfide, B₂S₃(s), reacts violently with water to form dissolved boric acid, H₃BO₃, and hydrogen sulfide gas.

Textbook Question

Write balanced chemical equations to correspond to each of the following descriptions: (c) Phosphine, PH₃(g), combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide.

Balance the following equations: (d) KOH(aq) + H3PO4(aq) → K3PO4(aq) + H2O(l)

Verified video answer for a similar problem:

Key Concepts

Balancing Chemical Equations

Acid-Base Reactions

Ionic Compounds and Solubility

Balance the following equations: (d) KOH(aq) + H₃PO₄(aq) → K₃PO₄(aq) + H₂O(l)