Answer:
The fire may grow bigger, depending on the gas.
Explanation:
If you expose more air to a small flame then it could grow larger because air keeps fire alive.
Answer:
2.14 × 10⁻³ molecules/RSP
3.31 × 10⁻³ molecules/ESP
Explanation:
Step 1: Calculate the number of moles of Acetaminophen per Regular Strength Pill (RSP)
A Regular Strength Pill has 1.29 × 10²¹ molecules of Acetaminophen per pill. To convert molecules to moles we will use Avogadro's number: there are 6.02 × 10²³ molecules in 1 mole of molecules.
1.29 × 10²¹ molecules/RSP × 1 mol/6.02 × 10²³ molecules = 2.14 × 10⁻³ molecules/RSP
Step 2: Calculate the number of moles of Acetaminophen per Extra Strength Pill (ESP)
An Extra Strength Pill has 1.99 × 10²¹ molecules of Acetaminophen per pill. To convert molecules to moles we will use Avogadro's number: there are 6.02 × 10²³ molecules in 1 mole of molecules.
1.99 × 10²¹ molecules/ESP × 1 mol/6.02 × 10²³ molecules = 3.31 × 10⁻³ molecules/ESP
Answer:
Explanation:
THE CORECT QUESTION
A 50.0 mL solution of 0.127 M KOH is titrated with 0.254 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCl.
SOLUTION
Get the concentration of the HCl first using titration formula
CA X V A / CB VB = NA/ NB
Equation of reation; KOH + HCl => KCl + H2O
CA = 0.254 M
CB = 0.127
VA = 1/0.254 = 3.937
CA (after the addition) = 0.127 x 50 / 3.937
= 1.612 M
But pH = - Log[hydrogen ion]
= -log 1.612
=
Answer:
Explanation:
Molarity is found by dividing the moles of solute by liters of solution.
We are given grams of a compound and milliliters of solution, so we must make 2 conversions.
1. Gram to Moles
We must use the molar mass. First, use the Periodic Table to find the molar masses of the individual elements.
- C: 12.011 g/mol
- H: 1.008 g/mol
- O: 15.999 g/mol
Next, look at the formula and note the subscripts. This tells us the number of atoms in 1 molecule. We multiply the molar mass of each element by its subscript.
6(12.011)+12(1.008)+6(15.999)=180.156 g/mol
Use this number as a ratio.
Multiply by the given number of grams.
Flip the fraction and divide.
2. Milliliters to Liters
There are 1000 milliliters in 1 liter.
Multiply by 2500 mL.
3. Calculate Molarity
Finally, divide the moles by the liters.
The original measurement has 2 significant figures, so our answer must have the same. That is the hundredth place and the 3 tells us to leave the 7.
1 mole per liter is also equal to 1 M.
Yes. As long as the ratio of solute and solvent is same for both solution, the solution has the same concentration. for example, solution A has 2 ml of water, and 1 ml of sucrose. Solution B has 4ml of water and 2ml of sucrose. Both has a ratio of water to sucrose by 2 : 1. they have the same concentration of 50% sucrose.
