Suppose you titrate 80.0 mL of 2.00 M NaOH with 20.0 mL of 4.00 M HCl....

Suppose you titrate 80.0 mL of 2.00 M NaOH with 20.0 mL of 4.00 M HCl. What is the final concentration of OH- ions.

Expert Solution

Number of moles of NaOH = M(NaOH) * V(NaOH)
                                                      = 2 M * 0.08 L
                                                        = 0.16 mol
Number of moles of HCl = M(HCl) * V(HCl)
                                                      = 4 M * 0.02 L
                                                        = 0.08 mol
HCL + NaOH -->NaCL + H2O
0.08 mol of each will react and neutralise each other

After Reaction :
Number of molesof NaOH remaining = 0.16 - 0.08 = 0.08 mol
Total volume= 80 mL+ 20mL =100 mL = 0.1 L
[OH-]=[NaOH]=Number of moles /Volume
= 0.08 / 0.1
= 0.8 M
Answer: final concentration of OH- ions= 0.8 M

queen_honey_blossom answered 8 months ago

What is the pH after the addition of 20.0 mL of 0.10 M NaOH to 80.0...

What is the pH after the addition of 20.0 mL of 0.10 M NaOH to 80.0 mL of a buffer solution that is 0.25 M in NH3 and 0.25 M in NH4Cl, (K b =1.8 x 10 −5 for NH3 )?

20.0 mL of 4.00 M HF and 40.0 mL of 2 M HCL are mixed. What...

20.0 mL of 4.00 M HF and 40.0 mL of 2 M HCL are mixed. What is the PH of the solution if the Ka of HF is 6.8 x 10^-4

Suppose you titrate 31.1 mL of 2.22 M ammonia, NH3, with 1.55 M HCl. a) How...

Suppose you titrate 31.1 mL of 2.22 M ammonia, NH3, with 1.55 M HCl. a) How many moles of NH3 are present in the original NH3 solution? b)what is the initial pH? c) what volume of HCl solution is required to reach the equivalence point? d) what is the pH at the equivalence point?

A quantity of 2.00 × 102 mL of 0.852 M HCl is mixed with 2.00 ×...

A quantity of 2.00 × 102 mL of 0.852 M HCl is mixed with 2.00 × 102 mL of 0.426 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.69°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions? H+(aq) + OH−(aq) → H2O(l)

Suppose we titrate 20.0 mL of 0.100 M HCHO2 (Ka = 1.8 × 10–4) with 0.100...

Suppose we titrate 20.0 mL of 0.100 M HCHO2 (Ka = 1.8 × 10–4) with 0.100 M NaOH. Calculate the pH. Before any base is added: pH = When half of the HCHO2 has been neutralized: pH = After a total of 15.0 mL of base has been added: pH = At the equivalence point: pH =

-If 35.00 mL of 0.0200 M aqueous HCl is required to titrate 30.00 mL of an...

-If 35.00 mL of 0.0200 M aqueous HCl is required to titrate 30.00 mL of an aqueous solution of NaOH to the equivalence point, the molarity of the NaOH solution is Blank 1 M. -20.00 mL of 0.510 M NaOH is titrated with 0.740 M H2SO4. Blank 1 mL of H2SO4 are needed to reach the end point.

If 36.0 mL of H3PO4 react exactly with 80.0 mL of 0.500 M NaOH, what is...

If 36.0 mL of H3PO4 react exactly with 80.0 mL of 0.500 M NaOH, what is the concentration of the phosphoric acid?

How many ml of 4.00 M HCl would you need to add to 500.0 ml of...

How many ml of 4.00 M HCl would you need to add to 500.0 ml of a 150. mM sodium acetate solution to make a buffer with a pH of 4.5? The pKa for acetic acid is 4.756.

70.0 mL base with 2.00 M molarity is added to 80.0 mL Oxalic acid with 1.80...

70.0 mL base with 2.00 M molarity is added to 80.0 mL Oxalic acid with 1.80 M molarity. The initial temperature is 20.0 °C and specific heat capacity is assumed to be the same as water (4.184 J/ g °C). Once the reaction reached thermal equilibrium, the temperature became 32.72°C. Find the enthalpy of neutralization for base.

You mix 100 mL of 1.0 M HCl with 100 mL of 1.0 M NaOH, both...

You mix 100 mL of 1.0 M HCl with 100 mL of 1.0 M NaOH, both initially at 25.0°C, into a coffee-cup calorimeter. The temperature of the reaction raises to 34.2°C. The heat capacity of the coffee-cup is 132 J/°C. What is the heat of the total reaction? What is it per mole of H2O (l) formed?

Question