A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for this solution. [Hint: Concentrated HCl is 38% HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO3 is 70.% HNO3 and has a density of 1.42 g/mL.]
Well, I'm not a scientist, but I can try to help you out with some humor! So, let's dive in and calculate some chemistry with a twist!
First of all, let's address the HCl and HNO3. Concentrated HCl... isn't it funny how it always wants to get straight to the point? You see, HCl is all about keeping things simple and straightforward! As for HNO3, it's like a nitric superstar, always bringing excitement and energy to the equation!
Now, to the calculations. We have 50.3 mL of concentrated HCl, which is 38% HCl by mass. So, we can convert the volume to mass using the density of 1.19 g/mL. That means we have... well, a whole lot of concentrated HCl! And trust me, concentrated HCl doesn't like to dilute itself with water, just like some people don't like to share their snacks!
Moving on to the HNO3, we have 16.6 mL of concentrated nitric acid, which is 70% HNO3 by mass. With a density of 1.42 g/mL, that makes for quite an explosive mixture! Just imagine the reaction when these two acids meet - it's like a chemical "KABOOM!"
Now, let's add 300 mL of water to the mix. Ah, water, the silent hero that dilutes all the chaos! But wait, there's more water to be added until we reach a final volume of 1.00 L. This journey feels like a marathon, but hey, there's nothing better than a refreshing glass of H2O after all the chemical commotion!
Alright, let's wrap this up and find the pH. To calculate the [H+], we need to know the concentration of H+ ions. And to figure that out, we need to consider the equilibrium constant... and maybe a little magic potion. Abracadabra! Voila! I'm just kidding, I'm no magician! But I can tell you that the concentration of H+ ions will increase with the amount of acid added.
As for [OH-], it will depend on the concentration of H+. Remember, they're frenemies - always acting against each other. But don't worry, they're not as dramatic as Taylor Swift and Katy Perry!
Lastly, the pH. The pH scale measures the concentration of H+ ions in a solution. So, as the concentration increases, the pH value decreases. It's like trying to balance on a see-saw - as one goes up, the other goes down! So, calculating the exact pH would require additional information about the concentration of H+ ions.
Well, I hope my humorous take on this chemistry problem at least made you smile! Remember, science may sometimes feel like a circus act, but with a little humor, we can all find the fun in it!
To calculate the [H+], [OH-], and pH of the solution prepared by adding hydrochloric acid, nitric acid, and water, we need to determine the number of moles of H+ and OH- ions present.
Step 1: Calculate the moles of HCl:
Mass of HCl = volume of concentrated HCl x density of HCl
= 50.3 mL x 1.19 g/mL
= 59.737 g
Moles of HCl = mass of HCl / molar mass of HCl
= 59.737 g / (1 g/mol + 35.453 g/mol)
= 1.656 mol
Step 2: Calculate the moles of HNO3:
Mass of HNO3 = volume of concentrated HNO3 x density of HNO3
= 16.6 mL x 1.42 g/mL
= 23.612 g
Moles of HNO3 = mass of HNO3 / molar mass of HNO3
= 23.612 g / (1 g/mol + 63 g/mol)
= 0.370 mol
Step 3: Calculate the total moles of H+ ions:
Total moles of H+ ions = moles of HCl + moles of HNO3
= 1.656 mol + 0.370 mol
= 2.026 mol
Step 4: Calculate the total volume of the solution:
Total volume of the solution = initial volume + volume of water added
= 300 mL + (1000 mL - 300 mL)
= 1000 mL
Step 5: Calculate the molarity of the H+ ions:
Molarity (M) = moles / volume (in liters)
= 2.026 mol / 1.00 L
= 2.026 M
Step 6: Calculate the concentration of OH- ions in water:
The concentration of OH- ions in water at 25°C is equal to 1 x 10^-14 M.
Step 7: Calculate the pH:
The relationship between [H+], [OH-], and pH is given by the equation:
pH + pOH = 14
pOH = -log10([OH-])
= -log10(1 x 10^-14)
= -(-14)
= 14
pH = 14 - pOH
= 14 - 14
= 0
Therefore:
[H+] = 2.026 M
[OH-] = 1 x 10^-14 M
pH = 0
To find the concentration of H+ ions, we first need to determine the number of moles of HCl and HNO3 added to the solution, and then calculate the concentration of H+ ions.
Step 1: Calculate the moles of HCl and HNO3 added.
The concentration of HCl is given as 38% HCl by mass. We can calculate the mass of HCl added as follows:
Mass of HCl = volume of HCl x density of HCl x mass % of HCl
Given that the volume of HCl added is 50.3 mL and the density of HCl is 1.19 g/mL, we can calculate the mass of HCl as follows:
Mass of HCl = 50.3 mL x 1.19 g/mL x 0.38 = 22.797 g
To find the moles of HCl, we need to divide the mass of HCl by its molar mass. The molar mass of HCl is 36.46 g/mol (1 mol of HCl contains 1 mol of H atoms with a mass of 1.01 g/mol and 1 mol of Cl atoms with a mass of 35.45 g/mol).
Moles of HCl = mass of HCl / molar mass of HCl
Moles of HCl = 22.797 g / 36.46 g/mol = 0.6258 mol
Similarly, using the same approach, we can calculate the moles of HNO3 added.
Mass of HNO3 = volume of HNO3 x density of HNO3 x mass % of HNO3
Mass of HNO3 = 16.6 mL x 1.42 g/mL x 0.70 = 16.54268 g
Molar mass of HNO3 = 63.02 g/mol
Moles of HNO3 = 16.54268 g / 63.02 g/mol = 0.2624 mol
Step 2: Calculate the final volume of the solution.
The final volume is given as 1.00 L. Therefore, the volume of water added is:
Volume of water = 1.00 L - 300 mL
Volume of water = 0.7 L = 700 mL
Step 3: Calculate the total moles of H+ ions.
To find the total moles of H+ ions, we need to sum up the moles of HCl and HNO3:
Total moles of H+ ions = moles of HCl + moles of HNO3
Total moles of H+ ions = 0.6258 mol + 0.2624 mol = 0.8882 mol
Step 4: Calculate the concentration of H+ ions.
The concentration of H+ ions is given in moles per liter (M). We can calculate the concentration using the formula:
[H+] = moles of H+ ions / volume of solution in liters
[H+] = 0.8882 mol / 1.00 L = 0.8882 M
Step 5: Calculate [OH-].
In a neutral solution, [H+] and [OH-] are equal. Since we have found [H+] to be 0.8882 M, [OH-] will also be 0.8882 M.
Step 6: Calculate the pH.
The pH of a solution can be calculated using the formula: pH = -log[H+]
pH = -log(0.8882) = 0.0519 (rounded to four decimal places)
Therefore, the concentration of [H+] is 0.8882 M, the concentration of [OH-] is 0.8882 M, and the pH of the solution is 0.0519.
First thing calculate the molarity of HCl and HNO3.
HCl: 1.19 g/mL x 1000 mL x 0.38/molar mass HCl = approx 12M but you need to do it more accurately.
HNO3: 1.42 g/mL x 1000 mL x 0.70/molar mass HNO3 = approximately 16M.
mol H^+ from HCl = 50.3 x 12M = ?
mol H^+ from HNO3 = 16.6 mL x 16 M = ?
Total mols H^+ = sum of the two.
(H^+) = moles/L soln.
Convert to OH^- and pH.