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How many grams are in 2 moles of nitric acid?
1+7+(8x3) =32 =32x2 (2 moles) =64
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
A nitric acid soulution is neutralized using sodium hydroxide how many grams of sodium hydroxide are needed to neutralize 2.50 L of 0.800 M Nitriric acid soulution?
Balanced equation first. HNO3 + NaOH >> NaNO3 + H2O Now, Molarity = moles of solute/volume of solution ( find moles HNO3 ) 0.800 M HNO3 = moles/2.50 Liters = 2 moles of HNO3 ( these reactants are one to one, so we can proceed to grams NaOH ) 2 moles NaOH (39.998 grams NaOH/1mole NaOH) = 79.996 grams of NaOH need to neutralize the acid. ( you do significant figures )
How many moles of sodium hydroxide are required to neutralize 20 mol of nitric acid?
The balanced chemical equation for the neutralization between sodium hydroxide (NaOH) and nitric acid (HNO3) is 1 mol of NaOH reacts with 1 mol of HNO3. Therefore, 20 moles of nitric acid would require 20 moles of sodium hydroxide to neutralize it.
What is the maximum mass of Nitric Acid which would be required to react with 0.35 grams of copper metal?
To determine the maximum mass of nitric acid required to react with 0.35 grams of copper metal, we need to calculate the moles of copper using its molar mass. Then, we use the balanced chemical equation between copper and nitric acid to find the mole ratio between them. Finally, we convert the moles of copper to moles of nitric acid and then to grams. The maximum mass of nitric acid needed can be determined as per the stoichiometry of the balanced chemical equation.
What is the molarity of a solution dissolve 0.31 grams of HNO3 in 300ml of water?
Molarity = moles of solute/Liters of solution ( get moles of HNO3 and 300 ml = 0.300 Liters ) 0.31 grams Nitric acid (1 mole HNO3/63.018 grams) = 0.004919 moles HNO3 Molarity = 0.004919 moles HNO3/0.300 Liters = 0.0164 M HNO3
How many grams are in 2 moles of nitric acid?
1+7+(8x3) =32 =32x2 (2 moles) =64
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
A nitric acid soulution is neutralized using sodium hydroxide how many grams of sodium hydroxide are needed to neutralize 2.50 L of 0.800 M Nitriric acid soulution?
Balanced equation first. HNO3 + NaOH >> NaNO3 + H2O Now, Molarity = moles of solute/volume of solution ( find moles HNO3 ) 0.800 M HNO3 = moles/2.50 Liters = 2 moles of HNO3 ( these reactants are one to one, so we can proceed to grams NaOH ) 2 moles NaOH (39.998 grams NaOH/1mole NaOH) = 79.996 grams of NaOH need to neutralize the acid. ( you do significant figures )
How many moles of sodium hydroxide are required to neutralize 20 mol of nitric acid?
The balanced chemical equation for the neutralization between sodium hydroxide (NaOH) and nitric acid (HNO3) is 1 mol of NaOH reacts with 1 mol of HNO3. Therefore, 20 moles of nitric acid would require 20 moles of sodium hydroxide to neutralize it.
What is the maximum mass of Nitric Acid which would be required to react with 0.35 grams of copper metal?
To determine the maximum mass of nitric acid required to react with 0.35 grams of copper metal, we need to calculate the moles of copper using its molar mass. Then, we use the balanced chemical equation between copper and nitric acid to find the mole ratio between them. Finally, we convert the moles of copper to moles of nitric acid and then to grams. The maximum mass of nitric acid needed can be determined as per the stoichiometry of the balanced chemical equation.
What weight of nitric acid can be produced from 18.5 gram of nitrogen dioxide?
To calculate the weight of nitric acid produced from 18.5 grams of nitrogen dioxide, you need to consider the stoichiometry of the reaction. The balanced chemical equation is: 2NO2 + H2O -> HNO3 + NO From the equation, we see that 2 moles of nitrogen dioxide produce 1 mole of nitric acid. First, convert 18.5 grams of nitrogen dioxide to moles, then use the mole ratio to find the moles of nitric acid produced. Finally, convert the moles of nitric acid to grams using the molar mass of nitric acid.
How many moles of HNO3 are required to react with 6 moles of Cu?
The balanced chemical equation for the reaction between copper (Cu) and nitric acid (HNO3) is: 3Cu + 8HNO3 -> 3Cu(NO3)2 + 2NO + 4H2O According to the equation, 8 moles of HNO3 are required to react with 3 moles of Cu. Therefore, to react with 6 moles of Cu, you would need 16 moles of HNO3.
How many moles of no2 will be obtained starting with 0.4 moles of nitric acid?
Starting with the formula: 2HNO3 --> H2O + NO2 If you have 0.4 moles of nitric acid (HNO3), you will get half the number of moles of NO2. So, you will have 0.2 moles of nitric acid.
A nitric acid solution is neutralized using sodium hydroxide How many grams of sodium hydroxide are needed to neutralize 2.50 L of 0.800 M nitric acid solution?
To neutralize the nitric acid, you need a 1:1 mole ratio of sodium hydroxide to nitric acid. First, calculate the moles of nitric acid in the solution using the formula Molarity = moles/volume. Then, use the mole ratio to find the moles of sodium hydroxide needed. Finally, convert this to grams using the molar mass of sodium hydroxide.
How many moles of NO2 will be obtained strating with 0.4 moles of nitric acid?
Starting with the formula: 2HNO3 --> H2O + NO2 If you have 0.4 moles of nitric acid (HNO3), you will end up with half the moles of nitrogen dioxide (NO2)...so you will have 0.2 moles.
How many moles of sodium hydroxide are required to neutralize 0.20 mol of nitric acid?
Balanced Equation. NaOH + HNO3 >> NaNO3 + H2O Now, Molarity = moles of solute/liters of solution 0.800M HNO3 + mol/2.50L mol of HNO3 = 2 2mol HNO3 (1mol NaOH/1molHNO3 )(39.998g NaOH/1mol NaOH ) = 79.996 grams
