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You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You...
final molarity of ammonium The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and...
final molarity of ammonium
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4, MM 98.00 g/mol) proceeds according to the following balanced eqation: 3NH2OH(aq) + H3PO4(aq)->3H20(1) + (NH4)3PO4(aq) What is the final molarity of the ammonium ion (NH4+. MM = 18.05 g/mol) when 25.0 mL of 1.20 molar ammonium hydroxide is reacted with 25.0 mL of 2.00 molar phosphoric acid?
urgent!!! The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4,...
urgent!!!
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4, MM = 98.00 g/mol) proceeds according to the following balanced eqation: 3NH4OH(aq) + H3PO4(aq) ->3H20(1) + (NH4)3PO4(aq) What is the final molarity of the ammonium ion (NH4+, MM = 18.05 g/mol) when 25.0 mL of 1.20 molar ammonium hydroxide is reacted with 25.0 mL of 2.00 molar phosphoric acid?
You need to prepare 200ml of a 0.4M solution of copper sulfate (CuSO4). You have 80mL...
You need to prepare 200ml of a 0.4M solution of copper sulfate (CuSO4). You have 80mL of a 0.5M CuSO4 solution and 100ml of 7.5% (w/v) CuSO4 solution. What volume of 7.5% CuSO4 and water needs to be added to the 80mL of 0.5M CuSO4 solution to make up 200mL of 0.4M CuSO4? Molar mass of CuSO4 = 159.609 g/mol % (weight/volume) means mass (in g) in volume (100mL)
You need to prepare a 2.10 M solution of sodium hydroxide (molar mass of sodium hydroxide=...
You need to prepare a 2.10 M solution of sodium hydroxide (molar mass of sodium hydroxide= 40.00 g/mol), but you only have 10 mL graduated cylinder and a 25 mL beaker. Complete the following sentences regarding the concentration of the prepared solution. 1. In order to prepare 10.0 mL (0.0100 L) solution of 2.10 M sodium hydroxide, a mass of ?? would be required. 2. When the solute and a total of 10.0 mL of water are both added into...
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.
A 3.82 L volume of gaseous ammonia, NH3 (g), at STP is bubbled through 100.0 mL...
A 3.82 L volume of gaseous ammonia, NH3 (g), at STP is bubbled through 100.0 mL water and reacts completely to form ammonium hydroxide, NH4OH (aq). a) What is the molar concentration of the resulting NH4OH (aq) solution? b) What mass of NH4OH is present in the 100.0 mL solution? c) How many moles of NH4OH would be present in 482 mL of a solution of the same concentration?
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.
A chemist would like to 800.0 mL of a 5.00 M solution of potassium hydroxide. What...
A chemist would like to 800.0 mL of a 5.00 M solution of potassium hydroxide. What mass of KOH is needed to make this solution? (Molar mass of KOH = 56.10 g/mol)
(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...
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=?
final molarity of ammonium
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4, MM 98.00 g/mol) proceeds according to the following balanced eqation: 3NH2OH(aq) + H3PO4(aq)->3H20(1) + (NH4)3PO4(aq) What is the final molarity of the ammonium ion (NH4+. MM = 18.05 g/mol) when 25.0 mL of 1.20 molar ammonium hydroxide is reacted with 25.0 mL of 2.00 molar phosphoric acid?
urgent!!!
The neutralization reaction between ammonium hydroxide (NH4OH, MM = 35.04 g/mol) and phosphoric acid (H3PO4, MM = 98.00 g/mol) proceeds according to the following balanced eqation: 3NH4OH(aq) + H3PO4(aq) ->3H20(1) + (NH4)3PO4(aq) What is the final molarity of the ammonium ion (NH4+, MM = 18.05 g/mol) when 25.0 mL of 1.20 molar ammonium hydroxide is reacted with 25.0 mL of 2.00 molar phosphoric acid?
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