IDNLearn.com provides a seamless experience for finding accurate answers. Find the answers you need quickly and accurately with help from our knowledgeable and dedicated community members.

We wish to determine how many grams of [tex]KNO _3[/tex] can form when 100 mL of [tex]0.40 M K _2 CrO _4[/tex] solution is added to excess [tex]AgNO _3[/tex].

[tex]\[ 2 AgNO _3( aq ) + K _2 CrO _4( aq ) \rightarrow Ag _2 CrO _4(s) + 2 KNO _3( aq ) \][/tex]

How many moles of [tex]K _2 CrO _4[/tex] are present in 100 mL of [tex]0.40 M K _2 CrO _4[/tex]?


Sagot :

To determine how many moles of [tex]\( K_2CrO_4 \)[/tex] are present in 100 mL of 0.40 M [tex]\( K_2CrO_4 \)[/tex], let's follow these steps:

1. Understand the given data:
- Volume of [tex]\( K_2CrO_4 \)[/tex] solution = 100 mL
- Concentration of [tex]\( K_2CrO_4 \)[/tex] solution = 0.40 M (moles per liter)

2. Convert the volume from mL to L:
- Volume in liters = [tex]\(\frac{100\text{ mL}}{1000}\text{ L} = 0.100\text{ L}\)[/tex]

3. Use the definition of molarity (M) which is moles per liter (mol/L) to find the number of moles of [tex]\( K_2CrO_4 \)[/tex]:
- Moles of [tex]\( K_2CrO_4 \)[/tex] = Molarity [tex]\(\times\)[/tex] Volume in liters
- Moles of [tex]\( K_2CrO_4 \)[/tex] = 0.40 M [tex]\(\times\)[/tex] 0.100 L = 0.040 moles

Therefore, the number of moles of [tex]\( K_2CrO_4 \)[/tex] present in 100 mL of 0.40 M [tex]\( K_2CrO_4 \)[/tex] is approximately [tex]\( 0.040 \)[/tex] moles.