Question

In: Chemistry

1. Calculate [OH?] for 1.7

1. Calculate [OH?] for 1.7

Solutions

Expert Solution

1)   [OH-] = 2 x 1.7 x 10-3 = 3.4 x 10-3 M

2) No.of moles of LiOH = 2.48/24 = 0.1

[OH-] =n x 1000/V = 0.1 x 1000/260

                                    = 0.384M

3) pOH = -log[OH-]

              = -log[0.384]

              = 0.41

pH = 14 - pOH = 14 - 0.41 = 13.59

4) NO.of moles of HClO3 = w/mw = 0.45/84 = 0.0053

                  [H+] = 0.0053/2.8 = 0.0018

pH = -log[H+] = -log[0.0018] = 2.74

5) M1V1 = M2V2

5 x 2 = M2 x 0.5 x 103

         M2 = 2 x 10-2

[H+] = 2x 10-2

pH = -log[2 x 10-2]

       = 1.69

6) [H+] = M1V1 + M2V2/(V1 + V2)

            = 2.5 x 10-2 x 60 + 1 x 10-2 x 160/( 60 + 160)

            = 1.4 x 10-2

pH = -log[1.4 x 10-2 ]

     = 1.85


Related Solutions

1) Calculate either [H3O ] or [OH
1) Calculate either [H3O ] or [OH
1. Calculate the pH of: A) 0.10 M ammonia (kb = 1.7 x 10 -5) ....
1. Calculate the pH of: A) 0.10 M ammonia (kb = 1.7 x 10 -5) . B) 0.15 M ammonium iodide (ka = 1.8 x 10 -5) . C) pure water D) 0.15 M hydrogen fluoride (ka = 4.2 x 10 -5) . E) 0.25 M hydrochloric acid. F) 0.15 M calcium hydroxide.
For each of the following strong base solutions,determine [OH], [H3O+], pH, pOH: 0.18M NaOH 1.7*10^-3m Ca(OH)2...
For each of the following strong base solutions,determine [OH], [H3O+], pH, pOH: 0.18M NaOH 1.7*10^-3m Ca(OH)2 5.0*10^-4M Sr(OH)2 8.8*10^-5M KOH
1) Calculate the solubility of Cu4(OH)6(SO4) in a basic solution containing 1.0 × 10-6 M OH-...
1) Calculate the solubility of Cu4(OH)6(SO4) in a basic solution containing 1.0 × 10-6 M OH- . (Ksp= 2.3 × 10-69)
Calculate [OH -] and pH for each of the following solutions. (a) 0.0034 M RbOH [OH-]...
Calculate [OH -] and pH for each of the following solutions. (a) 0.0034 M RbOH [OH-] =_________ M pH = _________ (b) 0.0872 g of KOH in 510.0 mL of solution [OH -] =__________ M pH = __________ (c) 79.8 mL of 0.00719 M Sr(OH)2 diluted to 900 mL [OH -] = __________ M pH = ____________ (d) A solution formed by mixing 64.0 mL of 0.000880 M Sr(OH)2 with 36.0 mL of 2.6 x 10-3 M RbOH [OH -]...
Calculate [OH -] and pH for each of the following solutions. (a) 0.0043 M KOH [OH-]...
Calculate [OH -] and pH for each of the following solutions. (a) 0.0043 M KOH [OH-] = _____  M pH = 11.63 (b) 0.0341 g of CsOH in 540.0 mL of solution [OH -] = 4.21e-4  M pH = 10.62 (c) 28.1 mL of 0.00187 M Ca(OH)2 diluted to 800 mL [OH -] = _____  M pH = 10.12 (d) A solution formed by mixing 71.0 mL of 0.000480 M Ca(OH)2 with 24.0 mL of 1.3 x 10-3 M KOH [OH -] =...
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...
a) Calculate the concentration of OH− in 1.54 M CH3CO2H. b) Calculate the concentration of CH3CO2H...
a) Calculate the concentration of OH− in 1.54 M CH3CO2H. b) Calculate the concentration of CH3CO2H in 0.0229 M CH3CO2H? c) Calculate the concentration of OH− in 0.0229 M CH3CO2H? d) Hippuric acid (HC9H8NO3), found in horse urine, has pKa=3.62. Calculate the concentration of HC9H8NO3 in 0.150 M hippuric acid?
1.Calculate the [H3O+] value of each aqueous solution. aspirin with [OH−]=1.4×10−11M. seawater with [OH−]=1.5×10−6M 2. To...
1.Calculate the [H3O+] value of each aqueous solution. aspirin with [OH−]=1.4×10−11M. seawater with [OH−]=1.5×10−6M 2. To calculate pH and use it as a measure of acidity. What is the pH of an aqueous solution with [H3O+] = 4×10−13M ? Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric acid. What is the molar concentration of H3O+ in a cola that has a pH of 3.120?
Calculate the pH of a 0.21 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x...
Calculate the pH of a 0.21 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x 10-9). Record your pH value to 2 decimal places. Calculate the pH of a 0.17 M solution of KNO2 (Ka for HNO2 = 4.0 x 10-4). Record your pH value to 2 decimal places.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT