So i need to calculate the pH of 50ml water (de-ionized) with 1 ml of 1M HCl. So the moles of HCl i think is .001 divided by the total amount of solution (.051). I get 0.0196, then i take the negative log of this number and it comes out to 1.71 roughly. Does this sound right? or did i miss something?
That looks ok to me.
Your approach to calculating the pH of the solution is correct. Let's go through the steps to double-check:
Step 1: Calculate the moles of HCl.
You correctly calculated the moles of HCl as 0.001 moles.
Step 2: Calculate the total volume of the solution.
You have 50 ml of water plus 1 ml of HCl, which gives a total volume of 51 ml or 0.051 L.
Step 3: Calculate the concentration of HCl.
Divide the moles of HCl (0.001 moles) by the total volume (0.051 L) to get the concentration of HCl: 0.0196 M.
Step 4: Calculate the pH.
To calculate the pH, take the negative logarithm (base 10) of the concentration of HCl. In this case, -log(0.0196) gives approximately 1.71.
So, your calculation is correct, and the pH of the solution should be around 1.71. Well done!