Home
Class 11
CHEMISTRY
What is the molarity of KI in a solution...

What is the molarity of KI in a solution that is `5.00%` KI by mass and has a density of `1.038g.cn^(-3)`?

A

`0.0301` M

B

`0.313` M

C

`0.500` M

D

`0.625` M

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Topper's Solved these Questions

  • MOLE CONCEPT, STOICHIOMETRY & CONCENTRATION TERMS

    GRB PUBLICATION|Exercise Percentage labelling of Oleum sample, volume strength of hyrogen Peroxide, ppm|23 Videos
  • MOLE CONCEPT, STOICHIOMETRY & CONCENTRATION TERMS

    GRB PUBLICATION|Exercise K. Eudiometry|74 Videos
  • MOLE CONCEPT, STOICHIOMETRY & CONCENTRATION TERMS

    GRB PUBLICATION|Exercise Experimental Methods|24 Videos
  • ISOMERISM

    GRB PUBLICATION|Exercise SUBJECTIVE TYPE|67 Videos
  • NOMENCLATURE AND CLASSIFICATION

    GRB PUBLICATION|Exercise Subjective Type|24 Videos

Similar Questions

Explore conceptually related problems

What is the molarity of HCl in a solution prepared by dissolving 5.5 g HCl in 200g ethanol if the density of solution is 0.79g/mL?

A solution of KI_3 in water contains

What is the molarity of HCl in a solution prepared by dissolving 5.5 g HCl in 200 g ethanol if the density of the solution is 0.79 g mL^(-1) ?

What is the molarity of H_(2)SO_(4) solution that has a density 1.84 g/c c at 35^(@) C and contains 98% by weight?

What is the molarity of H_(2)SO_(4) solution that has a density of 1.84g//cc and contains 98% by mass of H_(2)SO_(4) ?

A solution of KI_(3) in water contains :

An aqueous solution that is 30.0% NaOH by mass has a density of 1.33"g mL^(-1) .What is the molarity of NaOH in this solution?

Calculate the mole fraction, molality and molarity of HNO_(3) solution contaning 12.2% HNO_(3) .Given density of HNO_(3) = 1.038 g cm^(-3)

What is the molar mass of a gas that has a density of 5.66g L^(-1) at 35^(@)C and 745mm Hg?

GRB PUBLICATION-MOLE CONCEPT, STOICHIOMETRY & CONCENTRATION TERMS-Concentration Terms
  1. A solution of magnesium chloride that is 5.10% magnesium by mass has a...

    Text Solution

    |

  2. What volume of 0.108 M H(2)SO(4) is required to neutralize 25.0 mL of ...

    Text Solution

    |

  3. What is the molarity of KI in a solution that is 5.00% KI by mass and ...

    Text Solution

    |

  4. What is the concentration of the solution that results from mixing 40....

    Text Solution

    |

  5. What volume, in mL, of concentrated sulphuric acid (18.0"M H"(2)SO(4))...

    Text Solution

    |

  6. The bromide impurity in a 2.00 g sample of a metal nitrate is precipit...

    Text Solution

    |

  7. A 100 mL portion of 0.250 M calcium nitrate solution. What is the fina...

    Text Solution

    |

  8. What is the molarity of a 0.500 molal aqueous solution of calcium nitr...

    Text Solution

    |

  9. What volume of 0.150 M H(2)SO(4) would be required to completely neutr...

    Text Solution

    |

  10. A saturated aqueous solution of sucrose, C(12)H(22)O(11), contains 525...

    Text Solution

    |

  11. A 50.0 mL solution of 0.150 M HCl. Is mixed with 25.0 mL of 0.400 M HC...

    Text Solution

    |

  12. How many moles of ions are present in 250mL of a 4.4M solution of sodi...

    Text Solution

    |

  13. 40.0g of a solute is dissolved in 500mL of solvent to give a solution ...

    Text Solution

    |

  14. A 49.9g sample of barium hydroxide octahydrate, Ba(OH)(2).8H(2)O is di...

    Text Solution

    |

  15. What is the maximum mass of PbI(2) that can be precipitated by mixing ...

    Text Solution

    |

  16. Commercial vinegar is a 5.00% by mass aqueous solution of acetic acid,...

    Text Solution

    |

  17. What is the molarity of Na^(+) ions in a solution made by dissolving 4...

    Text Solution

    |

  18. What is the molarity of a hydorchlric acid solution if 20.00 mL of it ...

    Text Solution

    |

  19. A 65.25 g sample fo CuSO(4).5H(2)O (M=249.7) is dissolved in enough wa...

    Text Solution

    |

  20. How many moles of sulphate ions are in 100 mL of a solution of 0.0020 ...

    Text Solution

    |