Mass of NiCl2*6H2O. Please do steps.

Question

Question

science chemistry

Answer 1

Answer #1

Lets see the molecular mass of each

Ni = 58.693 g/mol

Cl = 35.453 g/mol

hence for Cl₂ = 2 x 35.453 = 70.906 g/mol

therefore for NiCl₂ = 58.693 + 70.906 = 129.599 g/mol

H = 1.0078 g/mol , then for H₂ = 2 x 1.0078 = 2.0156

O = 16 g/mol

therefore for H₂O = 2.0156 + 16 = 18.0156 g/mol

then for 6H₂O = 6 x 18.0156 = 108.0936 g/mol

Now lets add all to get Mass

= 129.599 + 108.0936

= 237.692 g/mol

So our Answer = 237.692 g/mol

Answer 2

Similar Homework Help Questions

Consider the reaction: NiCl2·6H2O + 3en → [Ni(en)3]Cl2 + 6H2O You start with 2.19 mol of...

Consider the reaction: NiCl2·6H2O + 3en → [Ni(en)3]Cl2 + 6H2O You start with 2.19 mol of NiCl2·6H2O and 5.80 mol of en (en = H2NCH2CH2NH2). What is the theoretical yield of [Ni(en)3]Cl2
Consider the reaction: NiCl2·6H2O + 3en → [Ni(en)3]Cl2 + 6H2O You start with 2.06 mol of...

Consider the reaction: NiCl2·6H2O + 3en → [Ni(en)3]Cl2 + 6H2O You start with 2.06 mol of NiCl2·6H2O and 5.46 mol of en (en = H2NCH2CH2NH2). What is the theoretical yield of [Ni(en)3]Cl2 ?
Mass of NiCl2 in 5 mL saturated solution = 2.73 g Solubility (g/L) of NiCl2 =...

Mass of NiCl2 in 5 mL saturated solution = 2.73 g Solubility (g/L) of NiCl2 = 546 g/L Molar solubility of NiCl2 = 4.44 M [Ni2+] = 4.44 M [Cl-] = 8.88 M Ksp for NiCl2 = 350.1 Why is it reasonable that the Ksp of NiCl2 should be so high?

In order to synthesize [Ni(NCS)2(PPh3)2], the following reagents are given: Ni(NO3)2 · 6H2O; KSCN; 1-butanol (C4H10O);...

In order to synthesize [Ni(NCS)2(PPh3)2], the following reagents are given: Ni(NO3)2 · 6H2O; KSCN; 1-butanol (C4H10O); Triphenylphosphine (PPh₃); EtOH; Et2O Please write the balanced equation for this synthesis reaction. In order to synthesize [NiCl2(PPh3)2], the following reagents are given: NiCl2 · 6H2O; Triphenylphosphine (PPh₃); CH3COOH; EtOH Please write the balanced equation for this synthesis reaction. Also, what are the byproduct salts produced in the two reactions?
2. You are in the lab; you dissolve 12.0 g NiCl2-6H2O (nickel chloride hexahydrate FW=237.69 g/mol);...

2. You are in the lab; you dissolve 12.0 g NiCl2-6H2O (nickel chloride hexahydrate FW=237.69 g/mol); you add a large excess of ammonia (NH3) in the form of concentrated ammonium hydroxide (NH4OH) and bring the solution to the mark in a 250 mL volumetric flask. The following nickel-amine complexes can be assumed to occur in the solution along with free nickel ion. Ni(NH3)2+ Ni(NH3)22+ (aq) Ni(NH3)3 2+ (aq) Ni(NH3)42 (aq) Ni(NH3)2+(aq) Ni(NH3)62+(aq) (a) Write a mass balance on Ni (for...
What volume of 0.150 M NiCl2 solution can be made from 35.7 g of NiCl2? The...

What volume of 0.150 M NiCl2 solution can be made from 35.7 g of NiCl2? The molar mass of NiCl2 is 129.6 g/mol. 0.041 L 0.544 L 2.42 L 1.84 L

Calculate the mass of nickel produced in 1.00 hr by the electrolysis of aqueous NiCl2 if...

Calculate the mass of nickel produced in 1.00 hr by the electrolysis of aqueous NiCl2 if the electrical current is 18.0 A.
Molar mass of Cu(NO3)2·6H2O molar mass of copper(II) nitrate, trihydrate

Molar mass of Cu(NO3)2·6H2O molar mass of copper(II) nitrate, trihydrate
please do it with steps and explanation!

please do it with steps and explanation!

1)Calculate the moles of ethylenediamine in 15 grams of a 25% by mass solution (i.e. in...

1)Calculate the moles of ethylenediamine in 15 grams of a 25% by mass solution (i.e. in 15 g of solution, 25% of the mass is ethylenediamine). .062 moles of C2H8N2 2. Calculate the moles of nickel(II) chloride in 3.5 g NiCl2·6H2O. .015 moles 3. Use the moles in questions 1 & 2 to determine the limiting reactant and excess reactant in your experiment today. Be sure to show all work.