-NO₂ 1) NaH THF 2) 3) dil. H3O+

Ph and pOh of 0.020m HNO3​

Will the following reaction yields a precipitate? yes or no   Pb(NO3)2(aq)  +  NaC2H3O2(aq) ->

4. (a) Calculate [H3O*] and [OH] for the solutions indicated: lemon juice, pH = 2.42 (1) (ii) household ammonia pH = 11.21 (iii) (iv) (v) phosphate buffer pH = 6.96 human urine pOH = 7.8 tomato juice pOH = 9.9

Q18

What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.

A neutralization reaction between KOH (aq) and H2SO4 (aq) would give which two products?

Calculate the concentration of HCO3 in an aqueous solution of 0.1120 M carbonic acid, H,CO3 (aq). [НСО3]%3D M.

Calculate the pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present. The pKb of ammonia solution is 4.75.

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)