Suppose you have 300 mL of 0.250 M solution of ammonium hydroxide. Ka=1.8x10^-5 A.What is the...
Suppose you have 300 mL of 0.250 M solution of ammonium hydroxide. Ka=1.8x10^-5
A.What is the pH solution?
B. You adjust pH solution to 9.70 so you will get ammonium chloride(molecular weight=53.49g/mol). What mass of the salt should you add? Assume volume doesn't change when NH4Cl is added.
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Suppose you have 300 mL of 0.250 M solution of
ammonium hydroxide. Ka=1.8x10^-5
A.What is the...
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of...
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You...
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You have 80 mL of a 0.5 M NHOH solution and 40 mL of a 7.5% (w/v) NH4OH solution. What volume of 7.5% NHOH and water needs to be added to the 80 mL of 0.5 M NH4OH solution to make up 200 mL of 0.4 M NH4OH? Molar mass of NH4OH 35.04 g/mol % (weight / volume) means mass (in g) in volume (100...
A buffer solution contains 0.341 M ammonium chloride and 0.291 M ammonia. If 0.0213 moles of potassium hydroxide are add...
A buffer solution contains 0.341 M ammonium chloride and 0.291 M ammonia. If 0.0213 moles of potassium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding potassium hydroxide) pH=?
(5 pts) At 20°C, a 0.376 M aqueous solution of ammonium chloride has a density of...
(5 pts) At 20°C, a 0.376 M aqueous solution of ammonium chloride has a density of 1.0045 g/mL. What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. 5) (5 pts) At 20°C, an aqueous solution that is 24.0% by mass in ammonium chloride has a density of 1.0674 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. i got 3.82...
Suppose 7.14g of potassium chloride is dissolved in 300.mL of a 0.60 M aqueous solution of...
Suppose 7.14g of potassium chloride is dissolved in 300.mL of a 0.60 M aqueous solution of ammonium sulfate. Calculate the final molarity of potassium cation in the solution. You can assume the volume of the solution doesn't change when the potassium chloride is dissolved in it. Round your answer to 3 significant digits.
Your supervisor asks you to prepare 474.00 mL of ammonium buffer solution 0.1 M with pH=...
Your supervisor asks you to prepare 474.00 mL of ammonium buffer solution 0.1 M with pH= 9.00, from a concentrated ammonia solution (16%w/w, d=0.98g/mL) and solid ammonium chloride (97% w/w). (MW of NH3 = 17.031 g/mol and FW of NH4Cl = 53.491 g/mol and pKa NH4+/NH3 =9.24). How many grams of the solid ammonium chloride do you need? Consider two decimal places for the answer.
Suppose 1.22 g of ammonium bromide is dissolved in 300. mL of a 59.0 m M...
Suppose 1.22 g of ammonium bromide is dissolved in 300. mL of a 59.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume of the solution doesn't change when the ammonium bromide is dissolved in it. Be sure your answer has the correct number of significant digits. [M OxO x | ?
Suppose 6.77g of ammonium chloride is dissolved in 50.mL of a 0.70 M aqueous solution of potassium...
Suppose 6.77g of ammonium chloride is dissolved in 50.mL of a 0.70 M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the ammonium chloride is dissolved in it. Be sure your answer has the correct number of significant digits.
1.0 L of a 1.2 M solution of formic acid (Ka=1.8x10-4) was prepared. What is the...
1.0 L of a 1.2 M solution of formic acid (Ka=1.8x10-4) was prepared. What is the pH of this solution? 1.8328 You are correct. Your receipt no. is 162-1608 Previous Tries Enough potassium formate was added to achieve a final potassium formate concentration of 1.7 M (assume the volume does not change). What is the pH of this new solution? 3.8960 You are correct. ceipt no. is 162-6598 Previous Tries 10 mL of 10 M NaOH is added to the...
Suppose 7.27g sodium chloride is dissolved in of 100 mL aqueous solution of 0.50 M ammonium...
Suppose 7.27g sodium chloride is dissolved in of 100 mL aqueous solution of 0.50 M ammonium sulfate. Calculate the final molarity of sodium cation in the solution. You can assume the volume of the solution doesn't change when the sodium chloride is dissolved in it. Round to 3 sig figs
A buffer solution contains 0.229 M ammonium chloride and 0.457 M ammonia. If 0.0568 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding hydroiodic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining A buffer solution contains 0.443 M ammonium chloride and 0.314 M ammonia. If 0.0313 moles of potassium hydroxide are added to 225...
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You have 80 mL of a 0.5 M NHOH solution and 40 mL of a 7.5% (w/v) NH4OH solution. What volume of 7.5% NHOH and water needs to be added to the 80 mL of 0.5 M NH4OH solution to make up 200 mL of 0.4 M NH4OH? Molar mass of NH4OH 35.04 g/mol % (weight / volume) means mass (in g) in volume (100...
Suppose 1.22 g of ammonium bromide is dissolved in 300. mL of a 59.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume of the solution doesn't change when the ammonium bromide is dissolved in it. Be sure your answer has the correct number of significant digits. [M OxO x | ?
1.0 L of a 1.2 M solution of formic acid (Ka=1.8x10-4) was prepared. What is the pH of this solution? 1.8328 You are correct. Your receipt no. is 162-1608 Previous Tries Enough potassium formate was added to achieve a final potassium formate concentration of 1.7 M (assume the volume does not change). What is the pH of this new solution? 3.8960 You are correct. ceipt no. is 162-6598 Previous Tries 10 mL of 10 M NaOH is added to the...
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