3 Pb(NO,) (aq) + 2 K,PO (aq) - Pb,(PO,)(s) + 6 KNO,(aq) Answer the following parts based on the above balanced chemical equation. Pb= 207.00 amu P= 31.00 amu 0 = 16.00 amu 1) How many grams of lead (Il) phosphate will be produced from the complete reaction of 212.5 mL of 0.1212 M solution of potassium phosphate? 2) How many milliliters of 0.2549 M lead (II) nitrate will be needed for the complete reaction of 112.9 mL of 0.2141 M solution of potassium phosphate

Complete (where necessary) and balance the following equation. Write the stoichiometric equation, then write the equation in ionic and net ionic form.  __ Cu(NO3)2 (aq) + __ NaOH (aq) → Cu(OH)2 (s) + __________

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!

Part 2 out of 3 (b) Balance the equation: Ba(OH)2(aq) + H3PO,(aq) → What is the ionic equation?

You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, provide the net ionic equation. KI+ Pb(NO3)2

If 355 mL of 0.325 M Pb(NO₃)₂ is added to 255 mL of 0.225 M K₃PO₄, how many moles of Pb₃(PO₄)₂ precipitate will be formed? The balanced equation is 3 Pb(NO₃)₂(aq) + 2 K₃PO₄(aq) → Pb₃(PO₄)₂(s) + 6 KNO₃(aq)

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP. How many grams of KHP are needed to exactly neutralize 20.5 mL of a 0.381 M barium hydroxide solution? Mass = grams KHC, H4O4

A student is trying to determine the concentration of an acetic acid (HC2H3O2) solution. They place 10.00 mL of the solution in a flask and titrate it with a 0.250 M NaOH solution. At the endpoint of the titration, they find that they have used 22.31 mL of the NaOH solution. Based on this information answer the following questions in the answer box provided. a) How many moles of NaOH are used to reach the endpoint? b) How many moles of acetic acid were neutralized by the NaOH added? c) What is the molar concentration (M) of the original acetic acid solution?

n the following reaction, when the equation is correctly balanced, what is the correct coefficient for sodium chloride? Pb(NO 3) 2( aq) + NaCl( aq) → PbCl 2 ( s) + NaNO 3( aq)     1     2     3     4     5

How many moles of Agl will be formed when 75.0 mL of 0.300 M AGNO: is completely reacted according to the balanced chemical reaction: 2 AGNO:(aq) + Cal:(aq) – 2 Agl(s) + Ca(NO:):(aq) STARTING AMOUNT *( ) 6.022 x 1028 0.0450 0.300 75.0 1 234.77 0.250 1000 169.88 22.5 0.001 0.0225 2 mL Agl mol AGNO: g Agl mol Agl mL AGNO: g AGNO: MAGNO. LAgl LAGNO: