PC15 (8) + H₂O(1) POCI, (1) + 2HCl(aq) When 62.57 g of phosphorus pentachloride reacts with excess water, what mass of hydrogen chloride will be produced? If needed, enter scientific notation with the "e". For example, 1.44×107 would be entered as 1.44e7. Answer: g HCI.

According to the following reaction, how many milliliters, mL of 0.152 M HCI is needed to neutralize 2.47 grams of Ca(OH)2? Just give the numerical value. The assumption is the answer is in milliliters, mL. Reaction: CaCl₂(aq) 2 HCl(aq) + Ca(OH)₂(aq) --- 2 H₂O(l) +

What mass (in kg) of H(OH) can be produced if 56mL of 0.982M H2C2O4•H2O solution reacts completely with excess NaOH? __ H2C2O4•H2O + __NaOH = __ Na2C2O4•H2O + __ H(OH)

27.

0.1061 g of dissolved oxalic acid dihydrate (molecular weight = 126.064 g/mole) is reacted with 20.0 mL of a sodium hydroxide solution. Calculate the molarity of the sodium hydroxide solution.  The balanced equation can omit the dihydrate from oxalic acid. Group of answer choices 0.0421 M 1.34 M 0.334 M 0.0842 M 0.669 M

If 2.00 grams of an unknown DIPROTIC acid (H2A) is titrated with 34.0 mL of 1.35 M NaOH, what is the molar mass (g/mol) of the diprotic acid? H2A+2NaOH⟶2H2O+Na2AH2A+2NaOH⟶2H2O+Na2A (Hint: See equation below in which mm is molar mass (units: g/mol), m is mass (unit: g), and mol isnumber of moles (unit: mol)). mmacid=macidmolacidmmacid=macidmolacid Molar Mass =  ___________   g/mol (input the numeric value only!) Remember: use correct significant figure rules. Significant figures always matter in Chemistry!

Question 34 of 42 If 32.0 g of NaOH is added to 0.550 L of 1.00 M Ni(NO,),, how many grams of Ni(OH), will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO,),(aq) → Ni(OH), (s) + 2 NaNO, (aq) 1 4 7 8. +/- x 100 MacBook 21

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Consider the unbalanced equation for the neutralization of acetic acid: HC2H3O2 (aq) + Ba(OH)2 (aq) ⟶ H2O (l) + Ba(C2H3O2)2 (aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 0.465 mole of HC2H3O2. Mol Ba(OH)2

solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.