The mass of a beaker is 5.333g. After 5.00 mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229 g. From the data, what is the measured density of the hydrochloric solution?
Can you please show me a step by step way to answer this. I am still totally confused...
Amy, I'm at a loss. Both Damon and I showed you how to work this problem. Somehow you punched in the wrong numbers or punched a wrong button on the calculator. The easiest way, short of me working the problem for you (which doesn't help you) is for you to show each step you followed and your answer. I will look for the error. That way we will know what is going wrong.
Sure! I'll break it down for you step by step:
Step 1: Determine the mass of the hydrochloric acid sample.
The mass of the beaker is given as 5.333g. The combined mass of the beaker and the hydrochloric acid sample is given as 11.229g. To find the mass of the hydrochloric acid sample, we subtract the mass of the empty beaker from the combined mass:
Mass of hydrochloric acid sample = Combined mass - Mass of beaker
Mass of hydrochloric acid sample = 11.229g - 5.333g
Mass of hydrochloric acid sample = 5.896g
Step 2: Calculate the volume of the hydrochloric acid solution.
The volume of the hydrochloric acid solution is given as 5.00 mL. Remember, the volume of a liquid is measured in milliliters (mL).
Step 3: Calculate the density of the hydrochloric acid solution.
Density is defined as the mass per unit volume. To find the density of the hydrochloric acid solution, we divide the mass of the hydrochloric acid sample by the volume of the solution:
Density = Mass of hydrochloric acid sample / Volume of hydrochloric acid solution
Density = 5.896g / 5.00mL
Density = 1.1792 g/mL
So, the density of the hydrochloric acid solution is 1.1792 g/mL.
I hope this helps! Let me know if you have any further questions.