If 60.13g of Nb(s) are added to 125.0ml of a 5.96mL of a 5.96 M solution of HClO4(aq), what is the mass of Nb(ClO4)5(aq) that is produced?

Suppose you took a 3.00 mL sample of HNO3 (aq) of an unknown concentration, and find that you have to add 20.30 mL of 0.106 M NaOH from your buret to neutralize the acid.  How many moles of OH- Ions are neutralized in this reaction?

Excess Na2SO4(aq) is added to a 2.43×102 mL sample of industrial waste containing Ba2+ ions. If 20.5 g of BaSO4(s) are precipitated from the reaction, what was the molar concentration of Ba2+ in the original sample?

If 16.0 mL of water are added to 31.5 mL of 0.586 M Ba(OH)2Ba(OH)2 (aq), what is the new solution molarity?

A noncarbonated soft drink contains an unknown amount of citric acid, H3 C6H5 O7. If 100. mL of the soft drink requires 35.96 mL of 0.0115 M NaOH to neutralize the citric acid completely, what mass of citric acid does the soft drink contain per 100. mL? The reaction of citric acid and NaOH is Mass= H3 C6H5O7 (aq) + 3 NaOH(aq) → Na3 C6H5O7 (aq) + 3 H₂O(l) g

A concentrated perchloric acid solution is 69.8% HCIO4 by mass and its density is 1.68 g mL-1. What volume (in litres) of the concentrated perchloric acid solution is needed to make 2.92L of 3.20 mol L-1 HCIO4(aq)? Molar masses, in g mol-1; HCIO4, 100.458 H2O, 18.016 0.447 L 0.0939 L 0.800 L 0.559 L 0.390 L Back: Question Menu

How many milliliters of 10.0 M HCl(aq) are needed to prepare 920.0 mL of 1.00 M HCl(aq)?

Vinegar is a solution of acetic acid, HC2H3O2, dissolved in water. A 5.84 g sample of vinegar was neutralized by 31.10 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar?

For each of the following reactions, suggest two soluble ionic compounds that, when mixed together in water, result in the net ionic equation given: (a) 2 Ag+ (aq) + CO3²¯ (aq) → Ag₂CO3(s) (b) Mg²+ (aq) + 2 OH¯(aq) → Mg(OH)₂(s), the suspension present in milk of magnesia 3+ (c) 3 Ca³+ (aq) + 2 PO2 (aq) → Ca3(PO4)2(s), gypsum, a component of concrete

A sample of 1.975 g oxalic acid dehydrate (H2C2O4 . 2H2O) was dissolved in enough water to make a 250.0 mL solution. What is the concentration of oxalic acid in the solution?In solid form, the dihydrate crystal lattice contains two water molecules for every oxalic acid molecule. The water molecules must be included as part of the molar mass. The molar mass of H2C2O4 * 2H2O is 126.064 g/mol. Oxalic acid is a diprotic acid (H2A). Write the balanced reaction for aqueous oxalic acid reacting with aqueous potassium hydroxide. If 20.00 mL of the oxalic acid solution described above is placed in a flask and then titrated with 0.1525 M potassium hydroxide, what volume of the potassium hydroxide solution would be required for a complete reaction?