How many g of C2H5NH3Cl will be needed to combine with 4.7 g of C2H5NH2 to produce 0.250 L of buffer solution at a pH of 10.00?

I can do this problem with mL and M but not w/out

convert the 4.7 g to moles by dividing by the molar mass

you have the L (convert to mL if needed)

then go for it

26.3g?

To solve this problem, you would need to use the molar masses of the compounds involved, along with knowledge of buffer solutions and pH calculations. Here's a step-by-step explanation of how you can approach this problem:

Step 1: Determine the balanced chemical equation for the reaction between C2H5NH2 (ethylamine) and C2H5NH3Cl (ethylammonium chloride) to form a buffer solution:

C2H5NH2 + HCl → C2H5NH3Cl

Step 2: Calculate the number of moles of C2H5NH2 using its molar mass. The molar mass of C2H5NH2 can be found by adding up the atomic masses of all the elements in the molecule (12.01 g/mol for C, 1.01 g/mol for H, and 14.01 g/mol for N):

Molar mass of C2H5NH2 = (2 * 12.01 g/mol) + (5 * 1.01 g/mol) + 14.01 g/mol = 45.08 g/mol

Number of moles of C2H5NH2 = Mass of C2H5NH2 (in grams) / Molar mass of C2H5NH2

Given: Mass of C2H5NH2 = 4.7 g

Number of moles of C2H5NH2 = 4.7 g / 45.08 g/mol = 0.104 moles

Step 3: Use the balanced chemical equation to determine the stoichiometry of the reaction. From the equation, it can be seen that one mole of C2H5NH2 reacts with one mole of C2H5NH3Cl.

Therefore, the number of moles of C2H5NH3Cl required is also 0.104 moles.

Step 4: Convert the volume of the buffer solution from liters to milliliters since we initially used mL and M in the problem statement.

Given: Volume of buffer solution = 0.250 L

Volume of buffer solution = 0.250 L * 1000 mL/L = 250 mL

Step 5: Use the Henderson-Hasselbalch equation to calculate the initial concentration of C2H5NH3Cl required to produce a solution with a pH of 10.00. The Henderson-Hasselbalch equation is given by:

pH = pKa + log([A-]/[HA])

Since we want a pH of 10.00, we need to determine the pKa of the C2H5NH3+/C2H5NH2 buffer system. Once you know the pKa value, you can use the equation to calculate the ratio [A-]/[HA]. This ratio will be equal to the concentration of C2H5NH3Cl divided by the concentration of C2H5NH2.

Step 6: Once you have the ratio [A-]/[HA], you can set up an equation to solve for the concentration of C2H5NH3Cl. The concentration of C2H5NH3Cl is equal to [A-], and the concentration of C2H5NH2 is equal to [HA].

Step 7: Convert the concentration of C2H5NH3Cl from moles per liter to grams per milliliter (g/mL) by using its molar mass:

Molar mass of C2H5NH3Cl = (2 * 12.01 g/mol) + (5 * 1.01 g/mol) + 14.01 g/mol + 35.45 g/mol = 109.61 g/mol

Step 8: Multiply the concentration of C2H5NH3Cl (in moles per liter) by its molar mass (in grams per mole) to get the grams of C2H5NH3Cl required.

Step 9: To summarize the solution, you would need to use 0.104 moles of C2H5NH3Cl to combine with 4.7 g of C2H5NH2 in order to produce 0.250 L (or 250 mL) of the buffer solution at a pH of 10.00.