How do I calculate the number of molecules in 6.00 ml of acetic anhydride, C4H6O3, if the density of acetic anhydride is 1.08 g/cm^3?

How many moles of Ba(OH)2 are present in 215 mL of 0.800 mol L-1 Ba(OH)2? Express your answer numerically in moles.

3. For each acid, name the anion bonded to hydrogen, then name the acid. Anion Name Acid Name (а) НBr (b) НF (c) H;S (d) HNO; (e) HC10;

What is the formula (solve for x) for the original hydrated sample of copper (II) sulphate? You weigh a sample of CuSO4 · XH2O. After you heat the sample, you find that the mass of the anhydrous salt is 1.47g. What is the value of x? CONTEXT Mass of just anhydrous compound = mass of anhydrous compound rod mass of beaker and 108.34g - 106.87g = 1.47g %3D %3D = original compound mass - anhydrous compound mass = 3.00g - 1.47g = 1.53g Mass of just water

If 465 g of Pb(NO3)2 (FW 331.21 g/mol) is added to a solution containing 215 g of K3PO4 (FW 212.27 g/mol), what mass, in g, of Pb3(PO4)2 (FW 811.54 g/mol) precipitate will be formed? The balanced equation is 3 Pb(NO3)2(aq) + 2 K3PO4(aq) → Pb3(PO4)2(S) + 6 KNO3(aq)

You have 235.5 g of Ba(OH)2   How many moles of barium hydroxide, Ba(OH)2, are present in 235.5  g? How many moles of barium ions are present? How many moles of hydroxide ions are present?

Consider the following chemical reaction: CaO(s) + H2O(l) ----------> Ca(OH)2 (aq) if 1.00 g calcium oxide is mixed with 2.00 g water, calculate grams of the product. CaO = 56.08 g/mole,  H2O = 18.02 g/mole,  Ca(OH)2 = 74.10 g/ mole

Aspirin can be prepared from salicylic acid (C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4 H6 O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C;H,O3 + C4H6O3 → C9HgO4 + C2H3O2 What is the theoretical yield, in grams, of aspirin (C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.06 g of salicylic acid with 3.71 mL of acetic anhydride? Type answer:

The organic salt tetrabutylammonium hexafluorophosphate is widely used as a non-aqueous electrolyte in electrochemistry. Its chemical formula is C16H36F6NP. Determine a) its molecular weight (in g/mol); b) the mass% of hydrogen; and c) the mass% of fluorine. Molar Mass: C=16, H=1, F=19, N=14, P=31

A chemist adds 2.00 L of a 5.9 × 10M mercury(II) iodide (HgI₂) solution to a reaction flask. Calculate the moles of mercury(II) iodide the chemist has added to the flask. Round your answer to 2 significant digits. mol 0 X S