How many grams of sodium hydroxide are needed to react with 50 grams of phosphoric acid?

To find out the number of grams of sodium hydroxide needed to react with 50 grams of phosphoric acid, we will first determine the balanced chemical equation for the reaction between sodium hydroxide (NaOH) and phosphoric acid (H3PO4).

The balanced chemical equation is:

3 NaOH + H3PO4 -> Na3PO4 + 3 H2O

From the equation, we can see that 1 mole of phosphoric acid reacts with 3 moles of sodium hydroxide.

To find the number of moles of phosphoric acid in 50 grams, we will use the formula:

moles = mass (in grams) / molar mass

The molar mass of phosphoric acid (H3PO4) is:
1(1) + 3(16) + 4(1) = 98 g/mol

So, moles of phosphoric acid = 50 g / 98 g/mol

Now, since the reaction ratio is 3:1 (sodium hydroxide to phosphoric acid), we need to multiply the moles of phosphoric acid by 3 to find the moles of sodium hydroxide required.

moles of sodium hydroxide = 3 * moles of phosphoric acid

Finally, to find the grams of sodium hydroxide needed, we multiply the moles of sodium hydroxide by its molar mass.

grams of sodium hydroxide = moles of sodium hydroxide * molar mass of sodium hydroxide

The molar mass of sodium hydroxide (NaOH) is:
23 + 16 + 1 = 40 g/mol

Now you can substitute in the values and calculate the answer:

moles of phosphoric acid = 50 g / 98 g/mol
moles of sodium hydroxide = 3 * moles of phosphoric acid
grams of sodium hydroxide = moles of sodium hydroxide * 40 g/mol

Once you calculate these values, you will have the number of grams of sodium hydroxide needed to react with 50 grams of phosphoric acid.