I'm having trouble solving this percentage concentration problem:

A student wants to make 5.00% solution of rubidium chloride using 0.377g of the substance. What mass of water will be needed to make the solution?

[g RbCl2/(g RbCl2 + g H2O)]x100 = 5.00

Solve for g H2O.

A day later I just notied a HUGH goof. Rubidium chloride is RbCl, NOT RbCl2. But that doesn't change the problem.

Well, it seems like you had a rubidium chloride dilemma, but no worries! Even if you're Rubidium Clueless, I'm here to lend a helping hand, or a clown-sized shoe, in this case.

So, let's solve this conundrum together. We know that the equation for the percentage concentration is:

[g RbCl/(g RbCl + g H2O)] x 100 = 5.00

Now, since the mass of rubidium chloride is given as 0.377g, we can assume that g RbCl is 0.377g. Let's substitute that into the equation:

[0.377/(0.377 + g H2O)] x 100 = 5.00

To solve for g H2O, we'll start by getting rid of the pesky percentage sign. Divide both sides of the equation by 100:

0.377/(0.377 + g H2O) = 0.05

Now, let's tackle the denominator. Cross-multiply and simplify the equation:

0.377 = 0.05(0.377 + g H2O)

0.377 = 0.01885 + 0.05g H2O

Next, let's isolate the g H2O term. Subtract 0.01885 from both sides:

0.377 - 0.01885 = 0.05g H2O

0.35815 = 0.05g H2O

Finally, divide both sides by 0.05 to find the mass of water, g H2O:

g H2O = 0.35815/0.05

g H2O = 7.163g

So, to make a 5.00% solution of rubidium chloride using 0.377g of the substance, you will need approximately 7.163g of water. Ta-da! Problem solved, and you're officially a chemistry clown.

No problem! Let's solve the problem step-by-step.

Step 1: Convert the percentage concentration to decimal form.
The given concentration is 5.00%, which means it is equal to 0.05 in decimal form.

Step 2: Calculate the mass of rubidium chloride needed.
The mass of rubidium chloride is given as 0.377g.

Step 3: Calculate the mass of water required.
Let's assume the mass of water needed is g H2O.

The total mass of the solution will be the sum of the mass of rubidium chloride and the mass of water:
Total mass = Mass of rubidium chloride + Mass of water

Since we want the final concentration to be 5.00%, we can write the equation as:
0.05 = (0.377g) / (0.377g + g H2O)

Step 4: Solve for g H2O.
To solve for g H2O, we can cross-multiply the equation:

0.05(0.377g + g H2O) = 0.377g

0.01885g + 0.05g H2O = 0.377g

Simplify the equation:

0.05g H2O = 0.377g - 0.01885g

0.05g H2O = 0.35815g

Divide both sides of the equation by 0.05:

g H2O = 0.35815g / 0.05

g H2O = 7.163g

So, you would need approximately 7.163 grams of water to make the 5.00% solution of rubidium chloride using 0.377g of the substance.

To solve this problem, you need to find the mass of water (g H2O) required to make a 5.00% solution of rubidium chloride.

First, let's understand the equation given:

[g RbCl/(g RbCl + g H2O)] x 100 = 5.00

This equation represents the percentage concentration of rubidium chloride in the solution. We need to find the mass of water (g H2O) required to make the final solution.

To solve for g H2O, we can rearrange the equation as follows:

g H2O = (g RbCl / (5.00/100)) - g RbCl

Now, let's substitute the given values into the equation:

g H2O = (0.377g / (5.00/100)) - 0.377g

Simplifying the expression:

g H2O = (0.377g / 0.0500) - 0.377g

g H2O = 7.54g - 0.377g

g H2O = 7.163g

Therefore, to make a 5.00% solution of rubidium chloride using 0.377g of the substance, you will need approximately 7.163g of water.