an auto mechanic spills 85 mL of 2.4 M H2SO4 solution from a rebuilt auto battery. how many mL of 1.2 M NaHCO3 must be poured on the spill to react completely with the sulfuric acid?

Write the equation and balance it.

H2SO4 + 2NaHCO3 ==> Na2SO4 + 2CO2 + 2H2O
(I think that's balanced but check it out.)
Convert 85 mL of 2.4 M H2SO4 to mols remembering that M x L = mols.
Convert mols H2SO4 to mols NaHCO3 using the coefficients in the balanced equation.
Then use M NaHCO3 = # mols/L. You know M of NaHCO3 and # mols, the only unknown is L.

Well, isn't this a bubbly situation! Let's do some chemical clowning to figure it out!

First, let's determine the number of moles of H2SO4 spilled. To do that, we multiply the volume (in liters) by the concentration (in moles per liter):
85 mL = 0.085 L
0.085 L * 2.4 mol/L = 0.204 moles of H2SO4

Now, let's find out how many moles of NaHCO3 are needed to react with the H2SO4. The balanced equation for the reaction is:
H2SO4 + 2 NaHCO3 -> Na2SO4 + 2 H2O + 2 CO2

From the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaHCO3. So, we need twice the number of moles of NaHCO3 compared to H2SO4.
0.204 mol * 2 = 0.408 moles of NaHCO3

Now, let's calculate the volume of 1.2 M NaHCO3 required to have 0.408 moles:
0.408 mol / 1.2 mol/L = 0.34 L = 340 mL

So, to clownishly react completely with the spilled sulfuric acid, the auto mechanic should pour 340 mL of 1.2 M NaHCO3 on the spill.

To determine how many mL of 1.2 M NaHCO3 is needed to react completely with the spilled sulfuric acid solution, we need to first find out the number of moles of H2SO4 spilled.

Step 1: Convert the volume of the spilled solution from mL to L:
85 mL = 85/1000 L = 0.085 L

Step 2: Calculate the number of moles of H2SO4:
moles = Molarity x Volume
moles = 2.4 M x 0.085 L = 0.204 moles

Step 3: Since the reaction between H2SO4 and NaHCO3 has a 1:2 stoichiometric ratio, we need twice the number of moles of NaHCO3 to fully react with the H2SO4.

Step 4: Calculate the number of moles of NaHCO3 needed:
moles NaHCO3 = 2 x moles H2SO4 = 2 x 0.204 moles = 0.408 moles

Step 5: Finally, use the molarity and moles of NaHCO3 to determine the volume required:
Volume = moles / Molarity
Volume = 0.408 moles / 1.2 M = 0.34 L

Step 6: Convert the volume from L to mL:
0.34 L = 0.34 x 1000 mL = 340 mL

Therefore, 340 mL of 1.2 M NaHCO3 should be poured on the spill to react completely with the sulfuric acid.

To find out how many mL of 1.2 M NaHCO3 is required to react completely with the spilled H2SO4, we can use the concept of stoichiometry and balanced chemical equation.

First, let's write the balanced chemical equation for the reaction between H2SO4 and NaHCO3:
H2SO4 + 2 NaHCO3 → Na2SO4 + 2 H2O + 2 CO2

From the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaHCO3.

Step 1: Convert the given volume of H2SO4 to moles:
Given volume of H2SO4 = 85 mL
Concentration of H2SO4 = 2.4 M

Using the equation: Moles = (Concentration × Volume) / 1000
Moles of H2SO4 = (2.4 M × 85 mL) / 1000 = 0.204 moles

Step 2: Based on the stoichiometry of the reaction, we know that for every 1 mole of H2SO4, we need 2 moles of NaHCO3.

So, moles of NaHCO3 needed = 2 × moles of H2SO4 = 2 × 0.204 = 0.408 moles

Step 3: Now, let's calculate the volume of 1.2 M NaHCO3 solution needed to get 0.408 moles:

Using the equation: Volume = (moles / Concentration) × 1000
Volume of NaHCO3 = (0.408 moles / 1.2 M) × 1000 = 340 mL

Therefore, approximately 340 mL of 1.2 M NaHCO3 solution must be poured on the spill to react completely with the sulfuric acid.