How many grams of Na2CO3 are present in 18.4 mL of a 34.0% Na2CO3 solution. The density of the solution is 1.10 g/mL.

1.10 g/mL x 18.4 mL x (34 g Na2CO3/100 g) = ?g Na2CO3

Well, if you're looking for a precise answer, you're definitely not going to get it from me! I'm a clown bot, remember? But I can try to give you a funny approximation if that's what you're looking for! So, let's see... If we take a leap of faith and assume that the density of your solution is actually the same as the density of my humor, which is pretty darn dense, then we can calculate it like this:

The volume of your solution is 18.4 mL and the density is 1.10 g/mL, so the solution weighs 20.24 grams (18.4 mL * 1.10 g/mL).

Since the solution is 34% Na2CO3, we can multiply the weight of the solution by 0.34 to get the weight of Na2CO3. That gives us a hilarious answer of approximately 6.89 grams (20.24 g * 0.34).

So there you have it. According to my clown calculations, there are about 6.89 grams of Na2CO3 in your 18.4 mL solution. But please, don't take my word for it and double-check with a more serious source before doing anything important!

To find the number of grams of Na2CO3 in the solution, we need to consider the following steps:

Step 1: Convert the volume of the solution from milliliters (mL) to grams (g) using the density.

Given:
Volume of the solution = 18.4 mL
Density of the solution = 1.10 g/mL

To convert mL to g, we multiply the volume (mL) by the density (g/mL):

18.4 mL × 1.10 g/mL = 20.24 grams

Step 2: Calculate the mass of Na2CO3 in the solution.

Given:
Percent concentration of Na2CO3 = 34.0%

The percent concentration (34.0%) represents the mass of Na2CO3 in 100 mL of the solution. So, we can set up the following proportion:

34.0 g Na2CO3 / 100 mL = x grams Na2CO3 / 20.24 grams

To solve for x, we cross-multiply and divide:

34.0 g Na2CO3 × 20.24 grams = 100 mL × x grams Na2CO3
x grams Na2CO3 = (34.0 g Na2CO3 × 20.24 grams) / 100 mL
x grams Na2CO3 = 688.16 grams / 100 mL
x grams Na2CO3 = 6.88 grams

Therefore, there are 6.88 grams of Na2CO3 present in 18.4 mL of a 34.0% Na2CO3 solution with a density of 1.10 g/mL.

To find the number of grams of Na2CO3 present in the solution, we need to use the following formula:

Mass of Na2CO3 = volume of solution (in mL) × concentration of Na2CO3 (in g/mL)

Let's break down the calculation step by step:

Step 1: Convert the given volume of the solution from mL to grams.
We are given the density of the solution, which is 1.10 g/mL. So, to convert 18.4 mL to grams, we can use the following equation:

Mass of solution = volume of solution × density of solution
Mass of solution = 18.4 mL × 1.10 g/mL

Step 2: Calculate the grams of Na2CO3 in the solution using the concentration of Na2CO3.
We are given that the solution is 34.0% Na2CO3, which means that for every 100 g of solution, there are 34.0 g of Na2CO3. We can convert this into a concentration in g/mL by dividing the concentration by 100.

Concentration of Na2CO3 = 34.0 g/100 g = 0.34 g/mL

Step 3: Substitute the values into the formula and solve.
Mass of Na2CO3 = volume of solution × concentration of Na2CO3
Mass of Na2CO3 = 18.4 mL × 0.34 g/mL

Now let's calculate the result:
Mass of Na2CO3 = 6.256 g

Therefore, there are 6.256 grams of Na2CO3 present in 18.4 mL of a 34.0% Na2CO3 solution.