what is the molarity of an HCL solution 28.6ml of a .175 m NaOH solution is needed to titrate a 15.0 ml sample of HCL solution
HCL(aq)+ NaOH(aq) -> NaCL(s) + H2O (l)
We know that number of moles of solute = Molarity of solution x Volume of solution (L)
So number of moles of NaOH=Molarity of NaOH x Volume of NaOH (L)
=0.175 M x 28.6 ml/1000 ml/L=5.005 x 10-3 mol
As per the given balanced chemical equation
1 mol NaOH reacts with 1 mol HCl
So 5.005 x 10-3 NaOH reacts with 5.005 x 10-3 mol HCl
So molarity of HCl solution=number of moles of HCl/volume of HCl solution (L)
=5.005 x 10-3 mol/15.0 ml/1000 ml/L=0.334 M
So molarity of HCl solution is 0.334 M
what is the molarity of an HCL solution 28.6ml of a .175 m NaOH solution is...
What is the molarity of a solution of HCl if 6.00 mL of the HCl solution is titrated with 26.8 mL of a 0.125 M NaOH solution? HCl(aq)+NaOH(aq)→H2O(l)+NaCl(aq)
What is the molarity of an HCl solution iſ 28.5 mL of 0.16 M NaOH are needed to neutralize 15.0 mL of the sample? MHCI
Determine the volume of 0.150 M NaOH solution required to neutralize 175 mL of a 0.66 M HCl solution. The neutralization reaction is NaOH(aq) + HCl(aq) → H2O(l) + NaCl(aq)
Data:
standaed HCL concentration : 0.1109 M
Accepted NaOH molarity: 0.0979 M
CALCULATIONS:
NOTE: Molarity (M) is #mole of solute in one L of solution
(units: mole solute/L solution)
HCl(aq) + NaOH(aq) ------------> NaCl(aq) + H2O (1)
1)Using the equation on the first page of this experiment solve
it for MNaOH (molarity of the now standardized base).
2)Calculate MNaOH for each run.
3)Find the average molarity of this NaOH solution.
4) Determine the % error.
What is the molarity of an HCl solution if 27.9 mL of 0.14 M NaOH are needed to neutralize 2.60 mL of the sample? _____M HCl
9. What is the hydroxide-ion concentration in a solution formed by combining 200 mL of 0.16 M HCl with 300. mL of 0.091 M NaOH at 25°C? HCl(aq) + NaOH(aq) + NaCl(aq) + H2O(1) 10. What is the pH of a solution prepared by dissolving 0.241 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 2.00 L? (R = 0.0821 L.atm/(K.mol)) (Use gas law equation to calculate Mole of HCl dissolved...
2. Calculate the molarity (M) of 30.0 g of NaOH in 350 mL of NaOH solution. Show all the step by step work: 3. Calculate the amount of solute, in moles, grams or milliliters, needed to prepare the following solutions. Show all the step by step solution: a. 1.00 L of a 3.00 M NaCl solution (moles of solute) b. 2.00 L of a 1.50 M NaOH solution (grams of solute) c. Milliliters of 1.50 M NaCl solution to obtain...
Determine the volume of 0.155 M NaOH solution required to neutralize each sample of hydrochloric acid. The neutralization reaction is: NaOH(aq) + HCl(aq) → H2O(l) + NaCl(aq) Part A 30 mL of a 0.155 M HCl solution Part B 50 mL of a 0.070 M HCl solutionPart C195 mL of a 0.925 M HCl solution
A 20.00 mL sample of HCl was titrated with the 0.022 M NaOH solution. To reach the endpoint required 23.72 ml of the NaOH. Calculate the molarity of the HCI. HCI + NaOH ----> NaCl + H2O Select one: O a. 0.026 M o b. 0.068 M o c. 0.039 M O d. 0.052 M
What is the molarity of a Ba(OH)2 solution if 813 mL is required to titrate 170 mL of 5.13 M HCl? Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2 H2O(l)