25cm3 of a solution of NaOH required 28cm3 of 1.0mol/dm3 H2SO4 to neutralise it:
a) write an equation for the reaction.
b) how many molesof H2SO4 were needed?
c) how many moles of NaOH were thus nuetralised?
a) Sure, let's write an equation for the reaction: NaOH + H2SO4 → Na2SO4 + H2O. Now we're ready to roll!
b) To calculate the number of moles of H2SO4 needed, we first need to convert the given volume of H2SO4 solution into liters. So, 28 cm3 is equivalent to 0.028 dm3. Since the concentration of H2SO4 is 1.0 mol/dm3, we multiply the volume by the concentration to get moles: 0.028 dm3 × 1.0 mol/dm3 = 0.028 moles of H2SO4.
c) Looking at the balanced equation, we can see that the ratio of NaOH to H2SO4 is 1:1. So, the number of moles of NaOH neutralized is also 0.028 moles.
Voilà! The reaction is balanced, the moles are calculated, and all is well in the world of chemistry.
a) The equation for the reaction between NaOH and H2SO4 is:
2NaOH + H2SO4 → Na2SO4 + 2H2O
b) To determine the number of moles of H2SO4 needed, we can use the equation:
Moles of solute = Volume of solution (in dm^3) × Concentration (in mol/dm^3)
Given that the volume of H2SO4 used is 28 cm^3 (which is equivalent to 0.028 dm^3) and the concentration of H2SO4 is 1.0 mol/dm^3, we can substitute these values into the equation:
Moles of H2SO4 = 0.028 dm^3 × 1.0 mol/dm^3
= 0.028 mol
Hence, 0.028 moles of H2SO4 were needed.
c) According to the balanced equation, for every 2 moles of NaOH, 1 mole of H2SO4 is required. Therefore, the number of moles of NaOH can be calculated using molar ratio:
Moles of NaOH = (Moles of H2SO4 ÷ 1) × (2 ÷ 1)
= 0.028 mol × 2
= 0.056 mol
Thus, 0.056 moles of NaOH were neutralized.
a) To write the equation for the reaction, we need to determine the substances involved and their chemical formulas. From the information given, we know that NaOH reacts with H2SO4. The chemical formulas for sodium hydroxide and sulfuric acid are NaOH and H2SO4, respectively. The equation for the reaction is:
NaOH + H2SO4 → Na2SO4 + H2O
b) To determine the number of moles of H2SO4 needed, we can use the equation:
moles = concentration (mol/dm3) × volume (dm3)
Given that the concentration of H2SO4 is 1.0 mol/dm3 and the volume is 28 cm3, we first need to convert the volume to dm3:
28 cm3 = 28/1000 dm3 = 0.028 dm3
Now, we can calculate the number of moles:
moles H2SO4 = 1.0 mol/dm3 × 0.028 dm3 = 0.028 moles
Therefore, 0.028 moles of H2SO4 were needed.
c) By stoichiometry, we know that the ratio of moles of H2SO4 to moles of NaOH is 1:1. This means that for every mole of H2SO4, one mole of NaOH reacts. Therefore, 0.028 moles of NaOH were thus neutralized.
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
I think for (b) you means how many mols H2SO4 were used. All of ot was meeded.
mols H2SO4 = M x L = ?
(c) Using the coefficients in the balanced equation, convert mols H2SO4 you had to mols NaOH neutralized.
(d) usually these problems want you to calculate the M of the NaOH.
That's M NaOH = mols NaOH/L NaOH