A 0.120-L sample of an unknown HNO3 solution required 29.1 mL of 0.200 M Ba(OH)2 for...

A 0.120-L sample of an unknown HNO3 solution required 29.1 mL of 0.200 M Ba(OH)2 for complete neutralization. What was the concentration of the HNO3 solution?

Expert Solution

Given Molarity of Ba(OH)₂ = 0.200 M

Volume of Ba(OH)₂ = 29.1 mL = 0.0291 L Sice 1 L = 1000 mL

So number of moles of Ba(OH)₂ is n = Molarity x volume in L

= 0.200 M x 0.0291 L

= 0.00582 mol

Ba(OH)₂ + 2HNO₃ Ba(NO₃)₂ + 2H₂O

According to the balanced equation ,

1 mole of Ba(OH)₂ reacts with 2 moles of HNO₃

0.00582 mole of Ba(OH)₂ reacts with 2x0.00582 = 0.01164 moles of HNO₃

So molarity of HNO₃ is ,

So the concentration of HNO₃ is 0.097 M

queen_honey_blossom answered 1 year ago

A 50.0 ml sample of 0.100 M Ba (OH)2 is treated with 0.100 M HNO3. Calculate...

A 50.0 ml sample of 0.100 M Ba (OH)2 is treated with 0.100 M HNO3. Calculate the ph after the addition of the following volumes of acid. a). 25 ml of HNO3 b). 50 ml of HNzo3 c). 75 ml of HNO3 d). 100 ml of HNO3 e). 125 ml of HNO3

A solution is made by mixing 12.5 g of Sr(OH)2and 40.0 mL of 0.200 M HNO3....

A solution is made by mixing 12.5 g of Sr(OH)2and 40.0 mL of 0.200 M HNO3. a. Calculate the concentration of OH− ion remaining in solution. b.Calculate the concentration of Sr2+ ion remaining in solution. c.Calculate the concentration of NO−3 ion remaining in solution. d. Is the resultant solution acidic or basic?

If 42.8 mL of 0.200 M HCl solution is needed to neutralize a solution of Ca(OH)2,...

If 42.8 mL of 0.200 M HCl solution is needed to neutralize a solution of Ca(OH)2, how many grams of Ca(OH)2 must be in the solution?

Calculate the pH of a 365.8-mL sample of 0.007 M Ba(OH)2 solution. Assume complete dissociation. Provide...

Calculate the pH of a 365.8-mL sample of 0.007 M Ba(OH)2 solution. Assume complete dissociation. Provide your answer to two decimal places and without units.

How many mL of 0.125 M Ba(OH)2 would be required to completely neutralize 75.0 mL of...

How many mL of 0.125 M Ba(OH)2 would be required to completely neutralize 75.0 mL of 0.845 M HCl? What is the pH of the solution at the equivalence point?

3. (A) A 25.0 mL sample of 0.103 M Ba(OH)2 was titrated with 0.188 M HClO4....

3. (A) A 25.0 mL sample of 0.103 M Ba(OH)2 was titrated with 0.188 M HClO4. Calculate the pH of the solution before the addition of any titrant and after the addition of 15.6, 27.4, and 38.1 mL of titrant.

Determine the [OH−] of a solution that is 0.120 M in CO32−.

2 HNO3(aq) + Ca(OH)2(aq) → Ca(NO3)2(aq) + 2 H2O(l) A 350 mL sample of 0.276 M...

2 HNO3(aq) + Ca(OH)2(aq) → Ca(NO3)2(aq) + 2 H2O(l) A 350 mL sample of 0.276 M HNO3 is partially neutralized by 125 mL of 0.120 M Ca(OH)2. Find the concentration of H+ (aq) in the resulting solution. A. 0.210 M B. 0.00632 M C. 0.203 M D. 0.0240 M E. 0.140 M

1. Calculate [OH−] for a solution formed by adding 5.00 mL of 0.120 M KOH to...

1. Calculate [OH−] for a solution formed by adding 5.00 mL of 0.120 M KOH to 20.0 mL of 7.1×10−2 M Ca(OH)2. 2. Calculate pH for a solution formed by adding 5.00 mL of 0.120 M KOH to 20.0 mL of 7.1×10−2 M Ca(OH)2. 3. Pyridine is a weak base that is used in the manufacture of pesticides and plastic resins. It is also a component of cigarette smoke. Pyridine ionizes in water as follows: C5H5N+H2O⇌C5H5NH++OH− The pKb of pyridine...

What volume of 0.075 M Ba(OH)2(aq) is required to completely neutralize 22.1 mL of 1.48 M...

What volume of 0.075 M Ba(OH)2(aq) is required to completely neutralize 22.1 mL of 1.48 M HNO3(aq)? A) 1.7 x 10–3 L B) 0.87 L C) 1.2 x 10–3 L D) 0.22 L E) 4.9 x 10–3 L

Question