Determine the pHpH of an HFHF solution of each of the following concentrations. The KAKA value of HFHF is 6.86.8 ×10−4×10−4. 4.90×10−2 MM Express your answer to two decimal places. |
Determine the pHpH of an HFHF solution of each of the following concentrations. The KAKA value...
Determine the pH of an HF solution of each of
the following concentrations.
HELP PLEASE.
Determine the pH of an HF solution of each of the following concentrations. 5.30x10^-2 Express your answer to two decimal places. Part C 2.00 x 10^-2 M Express your answer to two decimal places.
Use the Henderson-Hasselbalch equation to calculate the pHpH of each solution: a solution that is 0.14 MM in NH3NH3 and 0.18 MM in NH4Cl Express your answer using two decimal places.
Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8×10−4.) Part A 0.280 M Express your answer to two decimal places. Part B 4.70×10−2 M Express your answer to two decimal places. Part C 2.70×10−2 M Express your answer to two decimal places. Part D In which cases can you not make the simplifying assumption that x is...
Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that is small? (K, for HF is 6.8 x 10 ) Part A 0.260 M Express your answer to two decimal places. VALD + O 21 ? pH = Submit Request Answer Part B 5.00x10-2M Express your answer to two decimal places. 30 AL * O 31 ? pH = Submit Request Answer Part C 2.00x10-2M Express...
For each of the following strong base solutions, determine [OH−][OH−] and [H3O+][H3O+] and pHpH and pOHpOH. 1.) For 8.73×10−38.73×10−3 MM LiOHLiOH, determine [OH−][OH−] and [H3O+][H3O+]. Express your answers in moles per liter to three significant figures separated by a comma. 2.) For 1.10×10−21.10×10−2 MM Ba(OH)2Ba(OH)2, determine [OH−][OH−] and [H3O+][H3O+]. Express your answers in moles per liter to three significant figures separated by a comma. 3.) For 2.1×10−42.1×10−4 MM KOHKOH, determine [OH−][OH−] and [H3O+][H3O+]. Express your answers in moles per liter...
Determine the pH of an HNO2 solution of each of the following concentrations. A) 0.550M B) 0.100M C) 1.2x10^-2 M D) In which cases can you not make the simplifying assumption that x is small? only in (b) only in (a) in (b) and (c) in (a) and (b) PS: Express your answer to two decimal places
Part A Calculate the [H3O+][H3O+] and pHH of the following polyprotic acid solution: 0.390 MM H2C2O4H2C2O4. Express your answer using two significant figures. Part B Calculate the pHpH of this solution. Express your answer using two decimal places.
A 350.0 mLmL buffer solution is 0.150 molL−1molL−1 in HFHF and 0.150 molL−1molL−1 in NaFNaF. Ka(HF)=6.3×10−4 If the same volume of the buffer was 0.370 molL−1molL−1 in HFHF and 0.370 molL−1molL−1 in NaFNaF, what mass of NaOHNaOH could be handled before the pHpH rises above 4.00? Express your answer using two significant figures.
Amphetamine (C9H13N)(C9H13N) is a weak base with a pKbpKb of 4.2. Part A Calculate the pHpH of a solution containing an amphetamine concentration of 225 mg/Lmg/L . Express your answer to two decimal places.
1.Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D in the textbook). 0.435 M . 0.111 M . 3.79×10−2 M . 2.Consider two solutions, solution A and solution B. [H+] in solution A is 290 times greater than that in solution B. What is the difference in the pH values of the two solutions? Express your answer using two decimal places. 3.What volume of CO2 at 25...