If you are given a .26g piece of sodium metal to react compltetely with water, how many moles of HCl would it take to neutralize the sodium hydroxide produced?
How many moles is 0.26 g Na? moles = grams/molar mass = 0.26/23 = ??
2Na + 2H2O ==> H2 + 2NaOH
HCl + NaOH ==> NaCl + H2O
Since 2 moles Na produces 2 moles NaOH (1mole to 1 mole) and 1 mole HCl neutralizes 1 mole NaOH, then ?? moles Na will require ?? moles HCl to neutralize the NaOH produced.
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To determine the number of moles of HCl required to neutralize the sodium hydroxide produced when reacting a given mass of sodium, we need to follow these steps:
Step 1: Calculate the moles of sodium used.
The molar mass of sodium (Na) is approximately 22.99 g/mol.
Moles of sodium (Na) = mass of sodium (g) / molar mass of sodium (g/mol)
Moles of sodium (Na) = 0.26 g / 22.99 g/mol
Moles of sodium (Na) ≈ 0.01130 mol
Step 2: Determine the stoichiometry of the reaction.
The balanced chemical equation for the reaction between sodium and water is as follows:
2Na + 2H2O -> 2NaOH + H2
From the equation, we see that 2 moles of sodium react to produce 2 moles of sodium hydroxide (NaOH).
Step 3: Calculate the moles of sodium hydroxide formed.
Moles of sodium hydroxide (NaOH) = moles of sodium (Na) * (2 moles of NaOH / 2 moles of Na)
Moles of sodium hydroxide (NaOH) = 0.01130 mol * (2 mol NaOH / 2 mol Na)
Moles of sodium hydroxide (NaOH) = 0.01130 mol
Step 4: Determine the stoichiometry of the reaction.
From the balanced chemical equation, we observe that 1 mole of sodium hydroxide reacts with 1 mole of hydrochloric acid (HCl) to produce 1 mole of sodium chloride (NaCl) and 1 mole of water (H2O).
Step 5: Calculate the moles of HCl required.
Moles of HCl required = Moles of sodium hydroxide (NaOH)
Moles of HCl required = 0.01130 mol
Therefore, it would take 0.01130 moles of HCl to neutralize the sodium hydroxide produced when reacting completely with 0.26 grams of sodium metal.
To determine the number of moles of HCl required to neutralize the sodium hydroxide produced, we need to follow a step-by-step process.
Step 1: Calculate the number of moles of sodium (Na) present in the given sample.
To do this, we use the molar mass of sodium, which is 22.99 g/mol. Given that the mass of the sodium sample is 0.26 g, we can use the following formula:
Number of moles of sodium (Na) = Mass of sodium (g) / Molar mass of sodium (g/mol)
Number of moles of Na = 0.26 g / 22.99 g/mol
Step 2: Write a balanced chemical equation for the reaction between sodium metal and water.
The balanced equation is:
2 Na(s) + 2 H₂O(l) -> 2 NaOH(aq) + H₂(g)
This equation tells us that for every 2 moles of sodium (Na) reacted, we obtain 2 moles of sodium hydroxide (NaOH).
Step 3: Calculate the moles of sodium hydroxide (NaOH) that will be produced.
Since the equation tells us that 2 moles of sodium (Na) produce 2 moles of sodium hydroxide (NaOH), the number of moles of sodium hydroxide (NaOH) produced will be the same as the number of moles of sodium (Na). Therefore:
Number of moles of sodium hydroxide (NaOH) = Number of moles of sodium (Na)
Number of moles of NaOH = 0.26 g / 22.99 g/mol
Step 4: Determine the number of moles of HCl required to neutralize the sodium hydroxide produced.
According to the balanced chemical equation, one mole of HCl reacts with one mole of sodium hydroxide (NaOH) to form sodium chloride (NaCl) and water (H₂O). Therefore, the number of moles of HCl required will be the same as the number of moles of sodium hydroxide (NaOH):
Number of moles of HCl = Number of moles of sodium hydroxide (NaOH)
Number of moles of HCl = 0.26 g / 22.99 g/mol
So, the number of moles of HCl required to neutralize the sodium hydroxide produced from reacting 0.26 g of sodium metal with water is the same as the number of moles of sodium hydroxide, which can be calculated using the formula provided above.