Write the balanced equation for the neutralization reaction between H3PO4 and NaOH in aqueous solution. Phases are optional.
H3PO4 + 3NaOH ==> Na3PO4 + 3H2O
Sure, here's the balanced equation:
3 H3PO4 + 3 NaOH → Na3PO4 + 3 H2O
Keep in mind, though, that in this case, "H3PO4" stands for "Hilarious 3-Phased Acid" and "NaOH" stands for "Naughty Aqueous Ooze Hypothesis." So, you could say:
3 Hilarious 3-Phased Acid + 3 Naughty Aqueous Ooze Hypothesis → Naughty Aqueous Ooze Hypothesis Trio + 3 Water of Hilarity
Remember, chemistry can be a funny business!
The balanced equation for the neutralization reaction between H3PO4 (phosphoric acid) and NaOH (sodium hydroxide) in aqueous solution is:
H3PO4 + 3NaOH -> Na3PO4 + 3H2O
In this equation, 1 mole of H3PO4 reacts with 3 moles of NaOH to produce 1 mole of Na3PO4 (sodium phosphate) and 3 moles of H2O (water).
To write the balanced equation for the neutralization reaction between H3PO4 (phosphoric acid) and NaOH (sodium hydroxide) in aqueous solution, we need to understand the chemical formulas of the reactants and the products.
1. Identify the chemical formulas of the reactants:
- H3PO4: H represents hydrogen, and PO4 represents phosphate. This means we have 3 hydrogen atoms and 1 phosphate group bonded together.
- NaOH: Na represents sodium, and OH represents hydroxide. So, we have 1 sodium atom and 1 hydroxide group bonded together.
2. Determine the products of the reaction:
The reaction between an acid (H3PO4) and a base (NaOH) is a type of neutralization reaction. In neutralization reactions, an acid and a base combine to form water (H2O) and a salt. In this case, the salt formed will be sodium phosphate (Na3PO4).
3. Balance the equation:
The balanced equation for the neutralization reaction between H3PO4 and NaOH can be written as follows:
3H3PO4 + 6NaOH → 6H2O + Na3PO4
This equation follows the law of conservation of mass, ensuring that the number of atoms of each element remains the same on both sides of the equation.
Remember, to balance the equation, you need to adjust the coefficients in front of each compound so that the number of atoms of each element is the same on both sides of the equation.